Explanation:
The given reaction is as follows.
[tex]SO_{2} + O_{2} \rightarrow SO_{3}[/tex]
Now, balancing the given equation by putting appropriate coefficients.
[tex]2SO_{2} + O_{2} \rightarrow 2SO_{3}[/tex]
It is given that equimolar [tex]SO_{2}[/tex] and [tex]O_{2}[/tex]. Hence,
Therefore, during completion of the reaction,
[tex]SO_{2} + O_{2} \rightarrow SO_{3} + \frac{1}{2}O_{2}[/tex]
Temperature (T) = [tex]25^{o}C[/tex] = (25 + 273) K = 298 K
Pressure (P) = 1.75 atm
R (gas constant) = 0.0820 L atm/mol K
As on completion of reaction there is [tex]O_{2}[/tex] and [tex]SO_{3}[/tex] remains in the mixture. Therefore, molar mass of the mixture is equal to the sum of molar mass of
Total molar mass = [tex]O_{2} + SO_{3}[/tex]
= (32 + 80) g/mol
= 112 g/mol
Hence, according to the formula we will calculate the density as follows.
Density = [tex]\frac{P \times \text{molar mass}}{R \times T}[/tex]
= [tex]\frac{1.25 atm \times 112 g/mol}{0.0820 Latm/mol K \times 298 K}[/tex]
= 5.73 g/L
Thus, we can conclude that density of the product gas mixture is 5.73 g/L.
Answer:
d = 3.27g/L
Explanation:
[tex]2SO_{2} + O_2 => 2SO_3[/tex]
ICF table
2SO_{2} + O_2 => 2SO_3
initial 1 mol 1 mol 0 mol
change -1 mol 0.5 mol 1 mol
final 0 mol 0.5 mol 1 mol
calculate the mole fractions
[tex]X_O_2 = \frac{0.5 mol}{1.5 mol} = \frac{1}{3}\\\\X_S_O_3 = \frac{1 mol}{1.5 mol} = \frac{2}{3}\\[/tex]
[tex]\frac{n}{V} = \frac{P}{RT} = 0.0511 mol / L\\\\d = \frac{n}{RT} * X_O_2 * MM_O_2 + X_S_O_3 * MM_S_O_3\\\\d = (0.0511 mol/L) * (\frac{1}{3} mol * 32.0 g/mol + \frac{2}{3} * 80.06 g/mol)\\\\d = 3.27 g/L[/tex]
Dihydrogen dioxide decomposes into water and oxygen gas. Calculate the amounts requested if 1.34 moles of dihydrogen dioxide react according to the equation.
You must show all units.
a. Moles of oxygen formed
b. Moles of water formed
c. Mass of water formed
d. Mass of oxygen formed
Answer:
a) 0.67 moles of O2
b) 1.34 moles H2O
c) 24.15 grams of H2O
d) 21.44 grams O2
Explanation:
Step 1: Data given
Dihydrogen dioxide = H2O2
oxygen gas = O2
Moles H2O2 = 1.34 moles
Molar mass of H2O2 = 34.01 g/mol
Step 2: The balanced equation
2H2O2 → 2H2O + O2
Step 3: Calculate moles of H2O formed
For 2 moles H2O2 we'll have 2 moles H2O produced
For 1.34 moles H2O2 we have 1.34 moles H2O produced
This is 1.34 moles * 18.02 g/mol = 24.15 grams of H2O
Step 4: Calculate moles of O2 formed
For 2 moles H2O2 we'll have 1 mol O2 produced
For 1.34 moles H2O2 we'll have 1.34 /2 = 0.67 moles of O2 produced
This is 0.67 moles * 32.00 g/mol = 21.44 grams O2
. Naturally occurring element X exists in three isotopic forms: X-28 (27.979 amu, 92.21% abundance), X-29 (28.976 amu 4.70% abundance), and X-30 (29.974 amu 3.09% abundance). Calculate the atomic weight of X. a. 29.09 amu b. 28.09 amu c. 35.29 amu d. 86.93 amu e. 25.80 amu
Answer:
The correct answer is option b.
Explanation:
Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.
Formula used to calculate average atomic mass follows:
[tex]\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i[/tex] .....(1)
We are given:
Mass of isotope X-28 = 27.979 amu
Percentage abundance of isotope X-28 = 92.21%
Fractional abundance of isotope X-28 = 0.9221
Mass of isotope X-29 = 28.976 amu
Percentage abundance of isotope X-29 = 4.70%
Fractional abundance of isotope X-29 = 0.047
Mass of isotope X-30= 29.974 amu
Percentage abundance of isotope X-30 = 3.09%
Fractional abundance of isotope X-30 = 0.0309
Putting values in equation 1, we get:
[tex]\text{Average atomic mass of X}=\sum[(27.979 amu\times 0.9221)+(28.976 amu\times 0.047)+(29.974 amu\times 0.0309)][/tex]
[tex]\text{Average atomic mass of X}=28.09 amu[/tex]
The atomic weight of X is 28.09 amu.
The atomic weight of element X is calculated by considering the masses and abundances of its isotopes. By multiplying each isotope's mass by its abundance and summing up the products, the atomic weight of X can be determined to be 28.985 amu. Closest option to answer is option a.
Explanation:The atomic weight of an element is calculated by taking into account the masses and abundances of its isotopes. In this case, element X exists in three isotopic forms with different masses and abundances. To calculate the atomic weight of X, we multiply the mass of each isotope by its abundance and sum up the products.
Mass (amu) of X-28 multiplied by its abundance:(27.979 amu * 0.9221) = 25.699 amu
Mass (amu) of X-29 multiplied by its abundance:(28.976 amu * 0.047) = 1.361 amu
Mass (amu) of X-30 multiplied by its abundance:(29.974 amu * 0.0309) = 0.925 amu
Summing up the products:
25.699 amu + 1.361 amu + 0.925 amu = 28.985 amu
Therefore, the atomic weight of X is 28.985 amu.
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Show how to calculate the mass of a proton, neutron, and electron in kilograms using the data and the equality statement 1 amu = 1.66054 × 10-27 kg?
Answer:
Proton: m= 1.6726x10⁻²⁷ kg
Neutron: m= 1.6749x10⁻²⁷ kg
Electron: m= 9.1164x10⁻³¹ kg
Explanation:
We can calculate the mass of a proton, neutron, and electron using the following data:
mass of proton: 1.00728 amu
mass of neutron: 1.00867 amu
mass of electron: 5.49x10⁻⁴ amu
1 amu = 1.66054x10⁻²⁷ kg
Now, the mass of a proton, neutron, and electron in kilograms can be calculated using the next relation:
[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot particle's mass (amu) [/tex]
For the proton:
[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot 1.00728 amu = 1.6726 \cdot 10^{-27} kg [/tex]
For the neutron:
[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot 1.00867 amu = 1.6749 \cdot 10^{-27} kg [/tex]
For the electron:
[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot 5.49x10⁻⁴ amu = 9.1164 \cdot 10^{-31} kg [/tex]
I hope it helps you!
The masses of proton, neutron, and electron are approximately 1.6726 x 10-27 kg, 1.6749 x 10-27 kg and 9.109 x 10-31 kg, respectively. This is calculated by multiplying each particle's mass in Atomic Mass Units by the factor 1.66054 × 10-27 kg/amu.
Explanation:To calculate the mass of a proton, neutron, and electron in kilograms, we must know their masses in Atomic Mass Units (amu). We know that 1 amu = 1.66054 × 10
-27 kg. Using this we can get the masses as:
The mass of a proton is approximately 1.007 amu. So, converting this to kilograms we get 1.007 amu * 1.66054 × 10-27 kg/amu ≈ 1.6726 × 10-27 kg.The mass of a neutron is approximately 1.008 amu. Converting to kilograms, we get 1.008 amu * 1.66054 × 10-27 kg/amu ≈ 1.6749 × 10-27 kg.The mass of an electron is approximately 0.00055 amu. In kilograms, this becomes 0.00055 amu * 1.66054 × 10-27 kg/amu ≈ 9.10938356 × 10-31 kg.Learn more about Particle Mass Calculation here:https://brainly.com/question/26336269
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Choose the aqueous solution below with the lowest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable. Choose the aqueous solution below with the lowest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.
A. 0.075 m Li I
B. 0.075 m (NH4)3PO4
C. 0.075 m NaIO4
D. 0.075 m KCN
E. 0.075 m KNO2
Answer:
B. 0.075 m (NH4)3PO4
Explanation:
Our strategy here is to recall the van´t Hoff factor, i, for the colligative properties of electrolyte solutions which appears as the consequence that electrolytes disociate completely in their solutions in water.
Thus in this problem we need to determine i and then realize the one with the lowest freezing point will have the biggest i ( all the concentrations are equal) since
ΔTf = i m Kf
Substance van´t Hoff factor
Li I 2
(NH4)3PO4 4
NaIO4 2
KCN 2
KNO2 2
The correct answer is B. 0.075 m (NH4)3PO4
The aqueous solution with the lowest freezing point is 0.075 m (NH4)3PO4 because it dissociates into the highest number of particles, leading to the greatest freezing point depression.
Explanation:To find the aqueous solution with the lowest freezing point, we need to determine the effective concentration of solute particles after dissociation. Freezing point depression is larger for solutions with a higher number of dissolved particles. Therefore, we must consider the van't Hoff factor (i), which is the number of particles a compound dissociates into in solution. For example, LiI (i=2), NaIO4 (i=1), and KCN (i=2) will produce fewer particles than (NH4)3PO4, which will dissociate into four particles (i=4).
Given that the molal concentrations (m) are the same, the solution with the highest van't Hoff factor will have the highest concentration of particles and therefore, the lowest freezing point. Hence, solution B, 0.075 m (NH4)3PO4, with an effective concentration of 0.3 m (0.075 m × 4), will have the lowest freezing point.
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I just want to know the steps for how to solve this... literally have an exam tomorrow and I cannot stress enough how much I need to know this, ten points offered
Answer: 2,625.3 g AlCl3
Explanation: solution attached:
First balance the chemical equation then do basic stoichiometry.
What is the intensity in W/m2 of a laser beam used to burn away cancerous tissue that, when 91.0% absorbed, puts 540 J of energy into a circular spot 2.60 mm in diameter in 4.00 s?
Answer:
2.3x10⁷ W/m²
Explanation:
The intensity (I) of a laser is its potency (P) divided by the area (A) that it is affected. The potency is the energy applied (or absorbed) in a period, thus id 91.0% of the energy is absorbed, so:
E = 0.91*540 = 491.4 J
And,
P = E/t, where t is the time in seconds
P = 491.4/4.00
P = 122.85 J/s
P = 122.85 W
The are of a circular spot is:
A = (π/4)*d²
Where d is the diameter. Thus, with d = 2.60 mm = 0.0026 m
A = (π/4)*(0.0026)²
A = 5.31x10⁻⁶ m²
I = P/A
I = 122.85/5.31x10⁻⁶
I = 2.3x10⁷ W/m²
What is the type of strong chemical bond between carbon, hydrogen, and oxygen atoms in a single organic molecule?
Answer:
covalent bond
Explanation:
Covalent bond -
It is the type of interaction observed between two species , which share the electrons in order to attain stability , is referred to as covalent bond.
The shared electrons are referred to as the bonding pairs or the shared pairs .
Stability and completion of the octet is the driving force for the formation covalent bond.
The molecules of the organic compound usually shows this type bonding .
Like the bonds between - carbon , oxygen and hydrogen are covalent bonds.
As the temperature of a gas sample increases, the number of molecules and volume remaining constant, the pressure exerted by the gasA. increasesB. decreasesC. stays the same
Answer:
A. increases
Explanation:
According to the Gay-Lussac's law:-
Thus, at constant volume and number of moles, Pressure of the gas is directly proportional to the temperature of the gas.
P ∝ T
Also, it can be written as:-
[tex]\frac {P_1}{T_1}=\frac {P_2}{T_2}[/tex]
Thus, if the temperature is increased, the pressure exerted by the gas also increases.
Predict the shift in equilibrium position that will occur for each of the following reactions when the volume of the reaction container is increased.
A) 2COF2(g)⇌CO2(g)+CF4(g).
i) to the left.
ii) to the right.
iii) does not shift.
B) 2NO(g)+O2(g)⇌2NO2(g).
i) to the left.
ii) to the right.
iii) does not shift.
C) 2N2O5(s)⇌4NO2(g)+O2(g).
i) to the left.
ii) to the right.
iii) does not shift.
D) 2SO2(g)+O2(g)⇌2SO3(g).
i) to the left.
ii) to the right.
iii) does not shift.
E) PCl5(g)⇌PCl3(g)+Cl2(g).
i) to the left.
ii) to the right.
iii) does not shift.
Explanation:
Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.
This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.
Increase the volume:
If the volume of the container is increased, the pressure will decrease according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where increase in pressure is taking place. So, the equilibrium will shift in a direction where more number gaseous moles are present.
A) [tex]2COF_2(g)\rightleftharpoons CO_2(g)+CF_4(g)[/tex]
Number of gaseous moles on reactant side = 2
Number of gaseous moles on product side = 2
Equilibrium will not shift any direction as on both sides number of gaseous moles are same.
B) [tex]2NO(g)+O_2(g)\rightleftharpoons 2NO_2(g)[/tex]
Number of gaseous moles on reactant side = 3
Number of gaseous moles on product side = 2
Equilibrium will shift any left direction.
C) [tex]2N_2O_5(g)\rightleftharpoons 4NO_2(g)+O_2[/tex]
Number of gaseous moles on reactant side = 2
Number of gaseous moles on product side = 5
Equilibrium will shift any right direction.
D) [tex]2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)[/tex]
Number of gaseous moles on reactant side = 3
Number of gaseous moles on product side = 2
Equilibrium will shift any left direction.
E) [tex]PCl_5\rightleftharpoons PCl_3(g)+Cl_2(g)[/tex]
Number of gaseous moles on reactant side = 1
Number of gaseous moles on product side = 2
Equilibrium will shift any right direction.
Although all parts (postulates) of Dalton's atomic theory are important, which one of the postulates is crucial to explain the observations summarized by the Law of Definite Proportions?a. Atoms are very small.b. Atoms of the same elements have the same properties.c. Matter is composed of atoms. d. Atoms chemically combine with other atoms in fixed, whole-number ratios.
Answer:
The answer is D
Explanation:
Law of Definite Proportions states that a given compound always contain its component elements in fixed ratio (by mass) and does not depend on its source and/or method of preparation.
If one is to explain the law of definite proportions properly, then Dalton's fourth atomic theory comes to mind which states that atoms chemically combine with other atoms in fixed, whole number ratios.
The law of definite proportions suggests that compounds always contain its component elements in fixed ratio no matter the source, for example, oxygen makes up 8/9 of the mass of the sample of pure water regardless of the source while hydrogen makes up the remaining 1/9 of the mass. This generally shows that when oxygen and hydrogen combine in the ratio 8:1, water molecule will be formed as suggested by the Dalton Atomic Theory.
The Dalton's atomic theory postulate explaining the Law of Definite Proportions is 'Atoms chemically combine with other atoms in fixed, whole-number ratios.' This principle underlies consistent elemental proportions in compounds, such as the 1:8 ratio of hydrogen to oxygen in water.
Explanation:The postulate of Dalton's atomic theory that is vital to explain the observations summarized by the Law of Definite Proportions is: 'Atoms chemically combine with other atoms in fixed, whole-number ratios.'
This is crucial because the Law of Definite Proportions states that a given compound, regardless of the source or preparation method, will always consist of the same elements in the same proportion by mass.
For example, water (H2O) is always composed of 2 hydrogen atoms and 1 oxygen atom (fixed, whole-number ratio) regardless of the source. In water, the ratio of the mass of hydrogen to oxygen is always 1:8, which corroborates the Law of Definite Proportions.
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Explain why can two nonmetals bond together, but two metals cannot? A) Metals will only form covalent bonds. B) Nonmetals can share pairs of electrons and form ionic bonds. C) Nonmetals can share pairs of electrons and form covalent bonds. D) Metals will only share electrons and therefore cannot form ionic bonds.
Answer: C) Non-metals can share pairs of electrons and form covalent bonds
Explanation: The principal reason why it is non-metals that can form covalent bonds is because of their electronegativities. Electronegativity is the tendency of an atom to attract electrons towards itself.
The participating atoms in a covalent bond have to be able to hold the shared electron in place & it is this attraction towards the centre of each participating atom that holds the electrons in place. Metals aren't electronegative, they don't attract electrons towards each other, they'd rather even push the electrons away from themselves (electropositive) to be stable. The closest concept of metals to shared electrons is in metallic bonding, where metals push and donate their valence electrons to an electron cloud which is free to move around the bulk of the metallic structure. But this is nowhere near the type of bonding that exist in covalent bonds.
Answer:
C) Nonmetals can share pairs of electrons and form covalent bonds.
Explanation:
I’m having trouble with questions 1, 3, and 5.
Answer:
sorry i cant read sideways
Explanation:
A 5.34 g sample of an aluminum alloy is reacted with hydrochloric acid to produce aluminum chloride and hydrogen gas. At a temperature of 298 Kelvin and a pressure of 1.03 atm, a volume of 1.53 L of hydrogen gas is collected. Assuming that the hydrochloric acid only reacts with the aluminum in the sample, what is the percent of aluminum in the alloy sample? (Solid aluminum reacts with hydrochloric acid to produce aluminum chlo-1. 36.6 percent
2. 50.4 percent
3. 10.5 percent
4. 72.0 percent
5. 21.7 percent
Answer:
Option 5. 21.7 %
Explanation:
Let's think the reaction:
2Al (s) + 6HCl (l) → 3H₂ (g) + AlCl₃ (aq)
We have the data of hydrogen, we formed so let's apply the Ideal Gases Law equation to solve the amount of gas.
P . V = n . R . T
1.03 atm . 1.53L = n . 0.082 L.atm . 298K
(1.03 atm . 1.53L) / (0.082 L.atm . 298K) = n → 0.0645 moles of H₂
In the reaction, 3 moles of H₂ are produced by 2 moles of Al. Let's determine, how many moles of Al produced, the 0.0645 moles of H₂.
3 moles of H₂ were produced by 2 moles of Al
Then, 0.0645 moles of H₂ would be produced by (0.0645 .2)/3 = 0.043 moles.
If we convert the moles to mass, we can know the mass of Al in the alloy. (mol . molar mass)
0.043 m . 26.98 g/mol = 1.16 g
As the sample had a mass of 5.34 g, let's determine the % of Al.
(1.16 g / 5.34 g) . 100 = 21.7%
A chemical reaction in which two elements or radicals change places with two other elements or radicals is a _______ reaction. A. combination B. double replacement C. substitution D. decomposition
Answer: B
Double replacement reaction
Explanation:
after charcoal is added, the solution is filtered by hot gravity filtration. Why does the solution need to remain hot during the filtration to remove charcoal?
Answer:
The solution needs to remain hot during filtration in order to remove impurities and charcoal that are insoluble in the crystallization solvent, also to prevent crystals form prematurely on the paper filter or on the funnel stem.
The following substances dissolve when added to water. Classify the substances according to the strongest solute-solvent interaction that will occur between the given substances and water during dissolution.
1.ion-ion forces
2.dipole dipole forces
3.ion dipole forces
4.london dispersion forces
A. HF
B.CH3OH
C.CaCl2
D. FeBr3
HF and CH3OH exhibit dipole-dipole forces when dissolved in water because they both can form hydrogen bonds. CaCl2 and FeBr3 display ion-dipole forces in water because they are ionic compounds.
Explanation:When these substances are added to water, they exhibit different solute-solvent interactions due to their different properties.
HF (Hydrofluoric Acid): It exhibits dipole-dipole forces. HF can form hydrogen bonds, which is a type of dipole-dipole interaction, with water. CH3OH (Methanol): Similar to HF, methanol will also exhibit dipole-dipole forces when dissolved in water due to its ability to form hydrogen bonds. CaCl2 (Calcium Chloride): The interaction here are ion-dipole forces. Calcium chloride is an ionic compound and when added to water, it dissociates into ions which have strong ion-dipole interaction with water. FeBr3 (Iron (III) Bromide): This is an ionic compound and will also exhibit ion-dipole forces when dissolved in water.Learn more about Solvents and solutes here:https://brainly.com/question/31827211
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Consider two 5 L chambers. In one, there are 5.00 g O₂, and in the other there are 5.00 g He. Which has the higher pressure at room temperature?
A) O₂
B) Не
C) They have equal pressures
D) Not enough info
Answer:
He have higher pressure at room temperature.
Explanation:
It is given that both the gases are kept in 5 L chambers.
Therefore, volume is constant.
Also, they both are at room temperature, so temperature is also constant.
Now, number of moles of [tex]O_2[/tex] = [tex]\dfrac{Given\ mass}{Molecular \ mass}=\dfrac{5}{32}=0.16\ mol.[/tex]
Also, number of moles of He =[tex]\dfrac{Given\ mass}{Molecular \ mass}=\dfrac{5}{4}=1.25\ mol.[/tex]
Now, according to GAS LAW,
[tex]PV=nRT[/tex] ( all terms have their usual meaning).
In this case, V, R and T are constant.
So, pressure is directly proportional to n i.e number of moles.
So, moles of He is more than moles of [tex]O_2[/tex].
Therefore, He have higher pressure at room temperature.
Hence , this is the required solution.
The gas that has a higher pressure is He.
Number of moles of oxygen gas = 5.00 g /32 g/mol = 0.156 moles
From PV = nRT
P = ?
V = 5 L
n = 0.156 moles
T = 25 + 273 = 298 K
R = 0.082 atmLK-1mol-1
P = nRT/V
P = 0.156 moles × 0.082 atmLK-1mol-1 × 298 K/5 L
P = 0.76 atm
Number of moles of He = 5/4 g/mol = 1.25 moles
P = ?
V = 5 L
n = 1.25 moles
T = 25 + 273 = 298 K
R = 0.082 atmLK-1mol-1
P = nRT/V
P =1.25 moles × 0.082 atmLK-1mol-1 × 298 K/5 L
P = 6.11 atm
The gas that has a higher pressure is He.
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The radioactive decay of 99mTc to 99Tc MUST occur with the emission of:_______.
a) the combination of a beta particle and a gamma ray.
b) a gamma ray alone.
c) an alpha particle alone.
d) two beta particles.
Answer:
The answer is (B) A gamma ray alone
Explanation:
Technetium-99m decays through a process called isomeric transition involving the decay of 99mTc to 99TC via the release of gamma rays and low energy electron
In a reaction vessel, 17.6 g of solid chromium(III) oxide, Cr2O3, was allowed to react with excess carbon tetrachloride in the following reaction.
Cr2O3(s) + 3 CCl4(l) → 2 CrCl3(s) + 3 COCl2(aq)
Determine the percent yield of the reaction, given that the actual yield of chromium chloride, CrCl3, was 26.6 g. (The molar mass of Cr2O3 is 152.00 g/mol and the molar mass of CrCl3 is 158.35 g/mol.)
Answer:
72.53% is the yield of CrCl3
Explanation:
Given
Reaction:
Cr2O3(s) + 3 CCl4(l) → 2 CrCl3(s) + 3 COCl2(aq)
CCl4 is in excess and 17.6g Cr2O3 present
The reaction yields 26.6g of CrCl3
To Find:
% yields of the reaction
Also given
Molar mass of CrCl3 = 158.35g/mol
Molar mass of Cr2O3 = 152.00 g/mol
By the stoichiometry of the reaction
1 mole of Cr2O3 gives 2 moles of CrCl3
0r
1 x1 52 g of Cr2O3 gives 2x 158.35 g of CrCl3
= 1 52 g of Cr2O3 gives 316.70 g of CrCl3
17.6 g of Cr2O3 gives (17.6÷152) × 316.70 g CrCl3
= 36.67 g CrCl3
but actual yield is only 26.6g
so % yield is (26.6 ÷÷ 36.67) × 100
= 72.53% is the yield of CrCl3
Final answer:
To calculate the percent yield, the number of moles of chromium(III) oxide used was first determined, which was then used to find the theoretical yield of chromium chloride. The actual yield of chromium chloride is compared to this theoretical yield to find that the percent yield of the reaction is approximately 72.48%.
Explanation:
The student asked to calculate the percent yield of a chemical reaction involving chromium(III) oxide (Cr2O3) and carbon tetrachloride (CCl4). To find the percent yield, we need to compare the actual yield to the theoretical yield. First, we calculate the number of moles of Cr2O3 that react. With a molar mass of 152.00 g/mol, 17.6 g of Cr2O3 is equivalent to 0.1158 moles. According to the stoichiometry of the balanced equation, 1 mole of Cr2O3 produces 2 moles of CrCl3, which suggests that 0.1158 moles of Cr2O3 would yield 0.2316 moles of CrCl3. Using the molar mass of CrCl3 (158.35 g/mol), the theoretical yield of CrCl3 can be found as 0.2316 moles × 158.35 g/mol = 36.7 g.
Now, we calculate the percent yield using the actual yield (26.6 g) and the theoretical yield (36.7 g).
Percent Yield = (Actual Yield / Theoretical Yield) × 100 = (26.6 g / 36.7 g) × 100 ≈ 72.48%
Therefore, the percent yield of chromium chloride in the reaction is approximately 72.48%.
Gastric juices have a pH of 1 or 2. This would indicate which of the following?-neutral fluids, perfect for decomposition reactions-numerous H+ ions and a low pH-numerous OH- ions and a high pH-numerous OH- ions and a low pH
Answer:
Gastric juices have a pH of 1 or 2. This would indicate numerous H+ ions and a low pH
Explanation:
Highers concentrations of [H⁺] means very low pH.
pH = - log [H⁺]
Imagine this two concentrations:
[H⁺]₁ = 0.2 M
[H⁺]₂ = 0.0006 M
[H⁺]₁ > [H⁺]₂
pH₁ = - log 0.2 → 0.70
pH₂ = - log 0.0006 → 3.22
Then pOH₁ = 14 - 0.70 = 13.30
pOH₂ = 14 - 3.22 = 10.78
[OH⁻]₁ = 10^-pOH = 5.01×10⁻¹⁴
[OH⁻]₂ = 10^-pOH = 1.66×10⁻¹¹
As pH is so low, [OH⁻] is more and more lower.
A 6.00 L vessel contains 20.0 g of PCl3 and 3.15 g of O2 at 15.0 ∘C. The vessel is heated to 210 ∘C, and the contents react to give POCl3. What is the final pressure in the vessel, assuming that the reaction goes to completion and that all reactants and products are in the gas phase?
Answer: The final pressure in the vessel will be 0.965 atm
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] .....(1)
For phosphorus trichloride:Given mass of phosphorus trichloride = 20.0 g
Molar mass of phosphorus trichloride = 137.3 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of phosphorus trichloride}=\frac{20.0g}{137.3g/mol}=0.146mol[/tex]
For oxygen gas:Given mass of oxygen gas = 3.15 g
Molar mass of oxygen gas = 32 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of oxygen gas}=\frac{3.15g}{32g/mol}=0.098mol[/tex]
The chemical equation for the reaction of phosphorus trichloride and oxygen gas follows:
[tex]2PCl_3+O_2\rightarrow 2POCl_3[/tex]
By Stoichiometry of the reaction:
2 moles of phosphorus trichloride reacts with 1 mole of oxygen gas
So, 0.146 moles of phosphorus trichloride will react with = [tex]\frac{1}{2}\times 0.146=0.073mol[/tex] of oxygen gas
As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.
Thus, phosphorus trichloride is considered as a limiting reagent because it limits the formation of product.
By Stoichiometry of the reaction:
2 moles of phosphorus trichloride produces 2 moles of [tex]POCl_3[/tex]
So, 0.146 moles of phosphorus trichloride will produce = [tex]\frac{2}{2}\times 0.146=0.146mol[/tex] of [tex]POCl_3[/tex]
To calculate the pressure of the vessel, we use the equation given by ideal gas follows:
[tex]PV=nRT[/tex]
where,
P = pressure of the vessel = ?
V = Volume of the vessel = 6.00 L
T = Temperature of the vessel = [tex]210^oC=[210+273]K=483K[/tex]
R = Gas constant = [tex]0.0821\text{ L. atm }mol^{-1}K^{-1}[/tex]
n = number of moles = 0.146 moles
Putting values in above equation, we get:
[tex]P\times 6.00L=0.146mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 483K\\\\P=\frac{0.146\times 0.0821\times 483}{6.00}=0.965atm[/tex]
Hence, the final pressure in the vessel will be 0.965 atm
Answer:
The final pressure in the vessel is 1.13 atm
Explanation:
Step 1: Data given
Volume of the vessel = 6.00 L
Mass of PCl3 = 20.0 grams
Mass of O2 = 3.15 grams
Temperature = 15.0 °C
The vessel is heated to 210°C
Molar mass of PCl3 = 137.33 g/mol
Step 2: The balanced equation
2PCl3 + O2 → 2POCl3
Step 3: Calculate moles PCl3
MolesPCl3 = mass PCl3 / molar mass PCl3
Moles PCl3 = 20.0 grams / 137.33 g/mol
Moles PCl3 =0.146 moles PCl3
Step 4: Calculate moles O2
Moles O2 = 3.15 grams/ 32.0 g/mol
Moles O2 = 0.0984 moles O2
Step 5: Calculate the limiting reactant
PCl3 is the limiting reactant. It will completely be consumed(0.146 moles). So at completion there is no PCl3 remaining.
O2 is in excess. There will react 0.146/2 = 0.073 moles. There will remain 0.0984 - 0.073 = 0.0254 moles O2
Step 6: Calculate moles POCl3
For 2 moles PCl3 we need 1 mol O2 to produce 2 moles POCl3
For 0.146 moles PCl3 we'll have 0.146 moles POCl3
Step 7: Calculate final pressure
p*V = n*R*T
p = (n*R*T)/V
⇒ with n = the number of moles = 0.146 moles of POCl3 produced + 0.0254 moles O2 remaining = 0.1714 moles gas
⇒ with R = the gas constant = 0.08206 L*atm/mol*K
⇒with T = the temperature = 210 +273 = 483 Kelvin
⇒ with V = the volume = 6.00 L
p = (0.1714 *0.08206 * 483) / 6.00
p = 1.13 atm
The final pressure in the vessel is 1.13 atm
ANSWER NEEDED FAST 15 POINTS
WILL GIVE BRAINLIEST
How many grams of oxygen are required to burn 60 grams of ethane gas, C2H6?
2 C2H6 (g) + 7 O2(g) → 4 CO2 (g) + 6 H2O (g)
____grams
Answer:
224 grams of O₂
Explanation:
This is the reaction:
2 C₂H₆ (g) + 7 O₂(g) → 4 CO₂ (g) + 6 H₂O (g)
2 moles of ethene react with 7 moles of oxygen.
Let's convert the ethene's mass into moles (mass / molar mass)
60 g / 30 g/m = 2 mol
So, if 2 moles of ethene must react with 7 moles of O₂ and we have 2 moles, obviously we would need 7 moles of oyxgen.
Let's convert the moles to mass ( mol . molar mass)
7 m . 32 g/m = 224 grams
Answer: Mass of O2 is 224g
Explanation:
From the equation of the reaction, Ethane to oxygen is 2 to 7
While the molar masses respectively gives 30 and 32 g/mol
2 moles of methane gives 7 moles of O2;
60g/30=2moles for methane gives x/32 for O2;
Cross multiplying yields
7 x 2 = 2 x mass of O2/32
14 = 2x/32
Final answer gives 224 grams of oxygen
-----40 points-----
Magnesium is able to ____ copper, and copper is able to ____ magnesium.
Zinc is able to ____ magnesium, and magnesium is able to ____ zinc.
Copper is able to ____ zinc, and zinc is able to ____ copper.
In every blank, the options are "oxidize" and "reduce"
Answer:
1. Reduce
2. Oxidize
3. Oxidize
4. Reduce
5. Oxidize
6. Reduce
Explanation:
Answer:
1. Reduce, Oxidize
2.Oxidize, reduce
3.Reduce, Oxidize
Explanation:
Which of the following statements is true? Choose one: Na+ is the most plentiful positively charged ion outside the cell, while K+ is the most plentiful inside. K+ and Na+ are both excluded from cells. K+ and Na+ are present in the same concentration on both sides of the plasma membrane. K+ and Na+ are both maintained at high concentrations inside the cell compared to out. K+ is the most plentiful positively charged ion outside the cell, while Na+ is the most plentiful inside.
Answer:
Na+ is the most plentiful positively charged ion outside the cell, while K+ is the most plentiful inside.
Explanation:
Sodium ion and potassium ion play an important role in cellular metabolism. Na+ ion present in extracellular fluid while K+ ion is present in intracellular fluid.
Sodium ions are necessary for:
generation of nerve impulse
Heart activities
electrolyte balance
High or low concentration of sodium affects health.
Potassium ions are necessary for:
fluid and electrolyte balance
Na+ ion present in extracellular fluid while K+ ion is present in intracellular fluid.
Therefore, Na+ ion present in extracellular fluid while K+ ion is present in intracellular fluid.
The correct statement is that Na+ is the most plentiful positively charged ion outside the cell, while K+ is more plentiful inside, due to the function of the sodium-potassium pump in the plasma membrane of cells.
Explanation:The statement that is true among the given options is: Na+ is the most plentiful positively charged ion outside the cell, while K+ is the most plentiful inside. This arrangement is made possible through a process called the sodium-potassium pump, which is part of the plasma membrane of cells. The pump uses ATP to move 3 Na+ out of the cell and 2 K+ into the cell, which helps maintain the cell's resting potential. Therefore, outside of the cells, there is a higher concentration of Na+ ions, while inside the cells, K+ ions are more plentiful.
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A sample of concrete contains cement, gravel, crushed rocks, sand, and water. Each of these contains different metals and minerals and hence has different colors and different properties. Which term or terms could be used to describe this sample of concrete?a. Mixtureb. Heterogeneous mixturec. Homogeneous mixtured. Solutione. Pure chemical substancef. Compoundg. Element
Answer:
The answer to your question is a heterogeneous mixture
Explanation:
The Matter is classified as Pure substances and Mixtures
Pure substances are elements or compounds which are not mixed with more substances.
Mixtures are several elements or compounds together, mixtures can be homogeneous or heterogeneous.
Homogeneous mixtures are when the different components can be identified.
Heterogeneous mixtures are when the different components can be identified just by looking at the mixture.
In concrete we can identify the different components like gravel, sand, crushed rocks, etc, so concrete is a heterogeneous mixture.
Given the different molecular weights, dipole moments, and molecular shapes, why are their molar volumes nearly the same?
Answer:
Explanation:
Because most of the volume occupied by the substance is empty space.
Ammonia can be prepared by the reaction of magnesium nitride with water. The products are ammonia and magnesium hydroxide. When the equation is written and balanced, the coefficient of water is
1. 3
2. 2.
3. 6.
4. 1.
Answer:
Mg₃N₂ + 6H₂O → 2NH₃ + 3Mg(OH)₂
Coefficient of water is 6 (option 3)
Explanation:
The reaction is:
Mg₃N₂ + H₂O → NH₃ + Mg(OH)₂
Let's balance the reaction.
In reactant side we have 3 Mg, therefore in product side, we add 3 Mg to the hydroxide.
This change, modified the hydroxide, so now we have 6 O and 6 H, but we have in total 9 H (6 from the hydroxide + 3 from the ammonia)
As we have 2N, in reactant side, we must add 2 N to the ammonia, so now
we have 12 H in product side . We must complete with 6, the water so the H are ballanced.
In reactant side we have 6 O, therefore in product we must have 6 O (two O, in the OH but we have 3 moles, so in total we have 6 O) - BALANCED
The balance reaction is:
Mg₃N₂ + 6H₂O → 2NH₃ + 3Mg(OH)₂
The chemical reaction of magnesium nitride with water to form ammonia and magnesium hydroxide has a coefficient of 6 for water in the balanced equation.
Explanation:Preparing ammonia through the reaction of magnesium nitride with water yields ammonia and magnesium hydroxide. The balanced chemical equation for this reaction is: Mg3N2 + 6H2O → 3NH3 + 3Mg(OH)2. Thus, the coefficient of water in the balanced chemical equation is 6, which corresponds to option number 3 in your question.
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In the equation 2 H2 + O2 -> 2H2O, H2, O2, and H2O are all trace elements. Only H2O is a compound. Only H2 and O2 are compounds. H2, O2, and H2O are ALL elements. H2, O2, and H2O are ALL compounds.
Answer: only H2O is a compound
Explanation:
Nitrogen gas rreacts with hydrogen gas to form ammonia. At 200 celcius iun a closed container, 1 atm of nitrogen gas is mixed with 2 atm of hydogen gas. At equilibnrium, the toal pressure is 2 atm. Calcualate the value of [tex]K_p[/tex]?
Answer:
The value of Kp is 4
Explanation:
Step 1: Data given
The initial pressure of N2 = 1 atm
The initial pressure of H2 = 2 atm
Temperature = 200 °C
At equilibnrium, the toal pressure is 2 atm
Step 2: The balanced equation
N2(g) + 3H2(g) → 2NH3(g)
Step 3: The initial pressures
N2 = 1.0 atm
H2 = 2.0 atm
NH3 = 0 atm
Step 4: The partial pressures at equilibrium
For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3
There will react X moles of N2,
There will react 3X moles of H2
There will be produced 2X moles NH3
The partial pressure of N2 at the equilibrium is (1.0 -X)atm
The partial pressure of H2 at the equilibrium is (2.0 - 3X)atm
The partial pressure of NH3 at the equilibrium is 2X
The total pressure at the equilibrium = 2.0 atm
The total pressure = pN2 + pH2 +pNH3 = 2.0 atm
2.0 atm = (1.0-X) + (2.0 - 3X) + 2X
2.0 =3.0 -2X
X = 0.50
The partial pressure of N2 at the equilibrium is (1.0 -0.50) = 0.50 atm
The partial pressure of H2 at the equilibrium is (2.0 - 3*0.5) = 0.50 atm
The partial pressure of NH3 at the equilibrium is 2*0.5 = 1.0 atm
Step 5: Calculate Kp
Kp = pNH3 / (pN2)*(pH2)
Kp = 1.0 / (0.5*0.5)
Kp = 4
The value of Kp is 4
Balance the equation and identify the type of reaction for ? P4(s) + ? Ca(s) → ? Ca3P2(s). 1. 2; 6; 2 — decomposition 2. 2; 6; 2 — displacement 3. 1; 6; 2 — displacement 4. 1; 6; 2 — synthesis 5. 2; 6; 2 — synthesis 6. 1; 6; 2 — decomposition
Answer:
4. 1; 6; 2 — synthesis
Explanation:
Decomposition reaction is defined as the reaction in which a single large substance breaks down into two or more smaller substances.
[tex]AB\rightarrow A+B[/tex]
Single displacement reaction is defined as the reaction in which more reactive element displaces a less reactive element from its chemical reaction.
The reactivity of metal is determined by a series known as reactivity series. The metals lying above in the series are more reactive than the metals which lie below in the series.
[tex]A+BC\rightarrow AC+B[/tex]
Synthesis reaction is defined as the reaction in which smaller substances combine in their elemental state to form a larger substance.
[tex]A+B\rightarrow AB[/tex]
The unbalanced combustion reaction is shown below as:-
[tex]P_4+Ca\rightarrow Ca_3P_2[/tex]
On the left hand side,
There are 4 phosphorus atoms and 1 calcium atom
On the right hand side,
There are 2 phosphorus atoms and 3 calcium atoms
Thus,
Right side, [tex]Ca_3P_2[/tex] must be multiplied by 2 to balance phosphorus.
Left side, [tex]Ca[/tex] is multiplied by 6 so to balance the whole reaction.
Thus, the balanced reaction is:-
[tex]P_4+6Ca\rightarrow 2Ca_3P_2[/tex]
Thus, answer:- 4. 1; 6; 2 — synthesis