What is the angle between the carbon-chlorine bonds in the phosgene ( cocl2 ) molecule?

BaO..........................

The other reactant in the given reaction is [tex]\boxed{{\text{BaO}}}[/tex].

Further explanation:

A chemical reaction involves the rearrangement of the constituents of reactants to form new substances called products. Chemical reactions can be classified into the following five types:

1. Combination reactions

The chemical reactions where the combination of two or more reactants yields a single product are known as combination reactions. These are normally exothermic in nature.

Examples of combination reactions are as follows:

(a) [tex]{{\text{H}}_2} + {\text{C}}{{\text{l}}_2} \to {\text{2HCl}}[/tex]  

(b) [tex]{\text{CaO}} + {{\text{H}}_2}{\text{O}} \to {\text{Ca}}{\left( {{\text{OH}}} \right)_2}[/tex]  

2. Decomposition reactions

In these types of reactions, two or more products are produced from a single reactant. These are usually endothermic in nature.

Examples of decomposition reactions are as follows:

(a) [tex]2{{\text{H}}_2}{{\text{O}}_2} \to 2{{\text{H}}_2}{\text{O}} + {{\text{O}}_2}[/tex]  

(b) [tex]2{\text{NaCl}} \to {\text{2Na + C}}{{\text{l}}_2}[/tex]  

3. Displacement reactions

In these reactions, one of the reactants replaces another one due to its high reactivity. These reactions are also called replacement reactions.

Examples of displacement reactions are as follows:

(a) [tex]{\text{Cu}} + {\text{AgN}}{{\text{O}}_3} \to {\text{Ag}} + {\text{Cu}}{\left( {{\text{N}}{{\text{O}}_3}} \right)_2}[/tex]  

(b) [tex]{\text{C}}{{\text{l}}_2} + {\text{KBr}} \to {\text{B}}{{\text{r}}_2} + {\text{KCl}}[/tex]  

4. Double displacement reactions

In these reactions, ions of two compounds interchange with each other to form the product.

Examples of double displacement reactions are as follows:

(a) [tex]{\text{N}}{{\text{a}}_2}{\text{S}} + {\text{HCl}} \to {\text{NaCl}} + {{\text{H}}_2}{\text{S}}[/tex]  

(b) [tex]2{\text{KOH}} + {\text{Cu}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_2} \to 2{\text{KN}}{{\text{O}}_3} + {\text{Cu}}{\left( {{\text{OH}}} \right)_2}[/tex]  

5. Combustion reactions

These reactions occur when hydrocarbons are burnt in the presence of oxygen. Here, carbon dioxide and water are produced.

Example of combustion reactions are as follows:

(a) [tex]{\text{C}}{{\text{H}}_4} + {{\text{O}}_2} \to {\text{C}}{{\text{O}}_2} + {{\text{H}}_2}{\text{O}}[/tex]  

(b) [tex]{{\text{C}}_{10}}{{\text{H}}_{14}} + 12{{\text{O}}_2} \to 10{\text{C}}{{\text{O}}_2} + 4{{\text{H}}_2}{\text{O}}[/tex]  

One of the reactants is [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex] and the given reaction is a combination reaction. When BaO reacts with [tex]{{\text{H}}_{\text{2}}}{\text{O}}[/tex], it produces [tex]{\text{Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}}[/tex]. The reaction occurs as follows:

 [tex]{\text{BaO}} + {{\text{H}}_{\text{2}}}{\text{O}} \to {\text{Ba}}{\left( {{\text{OH}}} \right)_{\text{2}}}[/tex]

Therefore the other reactant in the given reaction is found to be BaO.

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Answer details:

Grade: High School

Chapter: Chemical reaction and equation

Subject: Chemistry

Keywords: types of reactions, combination reaction, decomposition reaction, double displacement reaction, combustion reaction, BaO, H2O, Ba(OH)2, reactants, products.

Answer :

Part 1 : Balanced reaction, [tex]3H_2(g)+N_2(g)\rightarrow 2NH_3(g)[/tex]

Part 2 : The theoretical yield of [tex]NH_3[/tex] gas = 440.96 g

Part 3 : The % yield of ammonia is 90.03 %

Solution : Given,

Mass of [tex]N_2[/tex] = 475 g

Molar mass of [tex]N_2[/tex] = 28 g/mole

Molar mass of [tex]NH_3[/tex] = 17 g/mole

Experimental yield of [tex]NH_3[/tex] = 397 g

Answer for Part (1) :

The balanced chemical reaction is,

[tex]3H_2(g)+N_2(g)\rightarrow 2NH_3(g)[/tex]

Answer for Part (2) :

First we have to calculate the moles of [tex]N_2[/tex].

[tex]\text{Moles of }N_2=\frac{\text{ Mass of }N_2}{\text{ Molecular mass of }N_2}=\frac{475g}{28g/mole}=16.96moles[/tex]

From the given reaction, we conclude that

1 moles of [tex]N_2[/tex] gas react to give 2 moles of [tex]NH_3[/tex] gas

16.96 moles of [tex]N_2[/tex] gas react to give [tex]\frac{2}{1}\times 16.96=33.92[/tex] moles of [tex]NH_3[/tex] gas

Now we have to calculate the mass of [tex]NH_3[/tex] gas.

[tex]\text{ Mass of }NH_3=\text{ Moles of }NH_3\times \text{ Molar mass of }NH_3[/tex]

[tex]\text{ Mass of }NH_3=(33.92moles)\times (17g/mole)=440.96g[/tex]

Therefore, the theoretical yield of [tex]NH_3[/tex] gas = 440.96 g

Answer for Part (3) :

Formula used for percent yield :

[tex]\% \text{ yield of }NH_3=\frac{\text{ Experimental yield of }NH_3}{\text{ Theoretical yield of }NH_3}\times 100[/tex]

[tex]\% \text{ yield of }NH_3=\frac{397g}{440.96g}\times 100=90.03\%[/tex]

Therefore, the % yield of ammonia is 90.03 %

From the balanced equation  3 moles of oxygen are produced from 2 molecules of potassium chlorate.

So the number of moles of oxygen from 1 mole of chlorate = 3/2 = 1.5.

By proportion  the number of moles produced from 6 moles of  the chlorate =

= 6 * 1.5  = 9 moles  (answer).

Considering the reaction stoichiometry, the correct answer is the last option: the total number of moles of O₂ produced by the decomposition of 6.0 moles of potassium chlorate is 9 moles.

The balanced reaction is:

2 KClO₃ → 2 KCl + 3 O₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

Then you can apply the following rule of three: if by stoichiometry 2 moles of KClO₃ produce 3 moles of O₂, 6 moles of KClO₃ will produce how many moles of O₂?

[tex]amount of moles of O_{2}=\frac{6 moles of KClO_{3} x 3moles of O_{2}}{2moles of KClO_{3} }[/tex]

amount of moles of O₂= 9 moles

Finally, the correct answer is the last option: the total number of moles of O₂ produced by the decomposition of 6.0 moles of potassium chlorate is 9 moles.

Learn more:

A chemical reaction absorbs energy which means it is endothermic reaction.

The reaction is endothermic if the energy of products is more than the energy of reactants.

The energy of products is more means that the bond energy of products is more than the bond energy of reactants.

so breaking of bond needs energy which is greater than the energy released in making of new bonds.

Enthalpy of reaction = Bond energy of reactants - Bond energy of products.

Answer:

its all of them

Explanation:

i got it off of edmentum

Salinity. Although everyone knows that seawater is salty, few know that even small variations in ocean surface salinity (i.e., concentration of dissolved salts) can have dramatic effects on the water cycle and ocean circulation. ... The weathering of rocks delivers minerals, including salt, into the ocean.

Answer:

salinity

Explanation:

I am not sure if this is what you are looking for, I have done a bit searching.

1 mol = 6..20 x 103 particles (atoms, molecules, formula units)

1 mol = molar mass/formula mass (Periodic Table)

1 mo = 22.4 L for a ga at STP

The three mole equalities are 1 mole = 6.20 x 103 particles,1 mole = molar mass/formula mass 1 mole = 22.4 L for a gas at STP.

Mole is defined as the unit of amount of substance . It is the quantity measure of amount of substance of how many elementary particles are present in a given substance.

It is defined as exactly 6.022×10²³ elementary entities. The elementary entity can be a molecule, atom ion depending on the type of substance. Amount of elementary entities in a mole is called as Avogadro's number.

It is widely used in chemistry as a suitable way for expressing amounts of reactants and products.For the practical purposes, mass of one mole of compound in grams is approximately equal to mass of one molecule of compound measured in Daltons. Molar mass has units of gram per mole . In case of molecules, where molar mass  in grams present in one mole  of atoms is its atomic mass.

Learn more about mole,here:

https://brainly.com/question/26416088

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Answer : The volume of neon gas will be, 7.99 liters.

Explanation : Given,

Mass of argon (Ar) gas = 27.1 g

Molar mass of argon = 39.95 g/mole

Volume of argon gas = 4.21 L

Moles of neon (Ne) gas = 1.29 mole

First we have to calculate the moles of argon gas.

[tex]\text{Moles of }Ar=\frac{\text{Mass of }Ar}{\text{Molar mass of }Ar}=\frac{27.1g}{39.95g/mole}=0.68moles[/tex]

Now we have to calculate the volume of neon gas.

According to the Avogadro's law, the volume of gas is directly proportional to the number of moles of gas at same pressure and temperature. That means,

[tex]V\propto n[/tex]

or,

[tex]\frac{V_1}{V_2}=\frac{n_1}{n_2}[/tex]

where,

[tex]V_1[/tex] = volume of argon gas

[tex]V_2[/tex] = volume of neon gas

[tex]n_1[/tex] = number of moles of argon gas

[tex]n_2[/tex] = number of moles of neon gas

Now we put all the given values in this formula, we get

[tex]\frac{4.21L}{V_2}=\frac{0.68mole}{1.29mole}[/tex]

[tex]V_2=7.99L[/tex]

Therefore, the volume of neon gas will be, 7.99 liters.

Answer:

C) Synthetic rubber has different monomers than natural rubber

Explanation:

Hello,

In this case, since statements A and B are correct due to the abundance of natural rubber and that both of them have the same properties making then suitable for several applications specially in the production of tires, belts, hoses, footwear and others, chemically, the best statement is C since the main monomers associated with synthetic rubber are derived from the petroleum byproducts such as styrene-butadiene whose condensation lead to the polymer forming the rubber. However, natural rubber is based on the isoprene (2-methyl-1,3-butadiene) as the promoting monomer whose polymerization lead to its formation.

Best regards.

True

Answer:

true

Explanation:

took test!

Answer : The maximum number of grams of [tex]PH_3[/tex] formed is, 8.955 g

Solution : Given,

Mass of phosphorous = 8.2 g

Mass of hydrogen = 4 g

Molar mass of [tex]P_4[/tex] = 123.6 g/mole

Molar mass of [tex]H_2[/tex] = 2.016 g/mole

Molar mass of [tex]PH_3[/tex] = 33.924 g/mole

The balanced chemical reaction is,

[tex]P_4(s)+6H_2(g)\rightarrow 4PH_3(g)[/tex]

First we have to calculate the moles [tex]P_4[/tex] and [tex]H_2[/tex]

[tex]\text{ Moles of }P_4=\frac{\text{ Mass of }P_4}{\text{ Molar mass of }P_4}=\frac{8.2g}{123.6g/mole}=0.066moles[/tex]

[tex]\text{ Moles of }H_2=\frac{\text{ Mass of }H_2}{\text{ Molar mass of }H_2}=\frac{4g}{2.016g/mole}=1.98moles[/tex]

From the reaction, we conclude that

1 mole of [tex]P_4[/tex] react with 6 moles of [tex]H_2[/tex]

0.066 moles of [tex]P_4[/tex] react with [tex]6\times 0.066=0.396[/tex] moles of [tex]H_2[/tex]

That means the [tex]H_2[/tex] is in excess amount and [tex]P_4[/tex] is in limited amount.

Now we have to calculate the moles of [tex]PH_3[/tex].

As, 1 mole of [tex]P_4[/tex] react to give 4 moles of [tex]PH_3[/tex]

So, 0.066 moles of [tex]P_4[/tex] react to give [tex]4\times 0.066=0.264[/tex] moles of [tex]PH_3[/tex]

Now we have to calculate the mass of [tex]PH_3[/tex]

[tex]\text{ Mass of }PH_3=\text{ Moles of }PH_3\times \text{ Molar mass of }PH_3[/tex]

[tex]\text{ Mass of }PH_3=(0.264moles)\times (33.924g/mole)=8.955g[/tex]

Therefore, the maximum number of grams of [tex]PH_3[/tex] formed is, 8.955 g

Answer:

ΔH = -22 kcal

Step-by-step explanation:

N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + 22 000 cal

Energy is on the right-hand side of the equation, so it is being released by the system.

The thermodynamic convention is that energy going out of a system is negative. Thus,

ΔH = -22 000 cal     Convert to kilocalories

ΔH = -22 kcal

A and B are both wrong, because you divide by 1000 to convert calories to kilocalories.

C is wrong, because the sign must be negative for an exothermic reaction.

The enthalpy change (ΔH) for the reaction N2(g) + 3H2(g) → 2NH3(g), which releases 22,000 calories, is -22,000 kcal.

The question is asking for the enthalpy change (ΔH) of the reaction where nitrogen gas (N2(g)) reacts with hydrogen gas (3H2(g)) to form ammonia (2NH3(g)). The enthalpy change is given in calories, and the options are either positive or negative, indicating an endothermic or exothermic reaction, respectively. The reaction as provided shows that it releases 22,000 cal, which means it's exothermic and ΔH should be negative. Therefore, the value of ΔH for the reaction N2(g) + 3H2(g) → 2NH3(g) is -22,000 kcal.

The enthalpy change for melting ice is called the entlaphy of fusion. Its value is 6.02 kj/mol. This means for every mole of ice we melt we must apply 6.02 kj of heat. We can calculate the heat needed with the following equation:

Q = N x ΔH

where:

Q  = heat

N  = moles  

ΔH  = enthalpy

In this problem we would like to calculate the heat needed to melt 35 grams of ice at 0 °C. This problem can be broken into three steps:

1. Calculate moles of water

2. multiply by the enthalpy of fusion

3. Convert kJ to J.

Step 1 : Calculate moles of water

[tex][ 75g ] x (\frac{1 mol}{18.02g} ) =[/tex]

Step 2 : Multiply by enthalpy of fusion

Q = N × ΔH  =  [ Step 1 Answer ] ×  6.02 =

Step 3 : Convert kJ to J

[tex][ Step 2 Answer ] x (\frac{1000j}{1kJ} ) =[/tex]

Finally rounding to 2 sig figs (since 34°C has two sig figs) we get

Q Would Equal ____

The correct option is d. 25, 050J of heat energy is required to melt 75g of ice at 0°C.

The mass of the ice given is 75g. To find the amount of heat energy required to melt this ice, we multiply the mass of the ice by the specific latent heat of fusion of water:

[tex]\[ Q = m \cdot L \][/tex]

Using the values provided:

[tex]\[ Q = 75 \text{g} \cdot 334 \text{J/g} \] \[ Q = 25,050 \text{J} \][/tex]

However, this value represents the heat energy required to melt 75g of ice into water at the same temperature (0°C). Since the ice is already at 0°C, we do not need to consider the energy required to raise its temperature from a lower value to 0°C.

Now, let's look at the options provided in the question:

 a. 4.45J: This is the energy required to raise the temperature of 1g of water by 1°C, which is not relevant to the melting process.

 b. 30.13J: This is a small amount of energy and seems incorrect for melting 75g of ice.

 c. 169,500J: This value is likely a misinterpretation of the correct calculation, as it could be the result of multiplying the mass of the ice by the specific latent heat of vaporization (which is about 2257 J/g for water), not fusion.

 d. 25,050J: This is the correct amount of heat energy required to melt 75g of ice at 0°C, as calculated above.

Consider the equation for calculating molarity: (no. of mole of solute)÷(volume of solution)

First, let's find the no. of mole of solute in AgNO3. As (no. of mole) = mass / molar mass

no. of mole of 85.0g of AgNO3 = 85.0/(107.9+14.0+16.0x3)

=0.5mol

Since the volume of the solution has to be in dm3, just divide the volume in cm3 by 1000 to get the volume in dm3.

Volume of solution = 500/1000

= 0.5 dm3

Therefore, the molarity is

0.5/0.5

=1.0M

The answer should be B.

It is in the center and everything surrounds it

Answer: The compound which is not an empirical formula is [tex]C_2N_2H_8[/tex]

Explanation:

Empirical formula is defined as the formula in which atoms in a compound are present in simplest whole number ratios.

For the given options:

Option A: [tex]C_3H_8O[/tex]

This compound is made by the combination of carbon, hydrogen and oxygen. The mole ratio of the elements are [tex]C:H:O::3:8:1[/tex]

Option B: [tex]C_2N_2H_8[/tex]

This compound is made by the combination of carbon, hydrogen and nitrogen. The mole ratio of the elements are [tex]C:N:H::2:2:8[/tex]

This ratio can be reduced to lowest numbers. The empirical formula of this becomes [tex]C_{2/2}N_{2/2}H_{8/2}=CNH_4[/tex]

Option C: [tex]Sb_2S_3[/tex]

This compound is made by the combination of tin and sulfur atoms. The mole ratio of the elements are [tex]SB:S::2:3[/tex]

Option D: [tex]BeCr_2O_7[/tex]

This compound is made by the combination of beryllium, chromium and oxygen. The mole ratio of the elements are [tex]Be:Cr:O::1:2:7[/tex]

Hence, the compound which is not an empirical formula is [tex]C_2N_2H_8[/tex]

Caffeine has the following percent composition: carbon 49.48%, hydrogen 5.19%, oxygen 16.48% and nitrogen 28.85%. Its molecular weight is 194.19 g/mol.

The percent composition of carbon in caffeine (C8H10N4O2) is calculated by dividing the total mass of carbon in one mole of the substance by its molar mass and multiplying by 100, which equals 49.48%.

The student has asked for the percent composition of carbon in caffeine, with the molecular formula C₈H₁₀N₄O₂. To calculate the percent composition, we first need to determine the molar mass of caffeine using the atomic masses of carbon (C), hydrogen (H), nitrogen (N), and oxygen (O). Then, we calculate the percentage by dividing the total mass of carbon in one mole of caffeine by the molar mass of caffeine and multiply by 100.

To calculate the percent composition of carbon in caffeine:

density = mass/volume

Answer:

Why is volleyball considered to be such a good aerobic exercise?

Explanation:

Answer:

D) is the correct answer on usatestprep

Explanation:

(a) A material that can be melted and reformed at a low temperature.

1)ionic solid      

2) molecular solid  

3)metallic solid  

4)covalent network solid

(b) A material that can be drawn into long, thin wires.  

1)ionic solid  

2)molecular solid  

3)metallic solid

4)covalent network solid

(c) A material that conducts electricity when molten.

1)ionic solid  

2)molecular solid  

3)metallic solid  

4)covalent network solid  

(d) An extremely hard material that is non-conductive.

1)ionic solid  

2)molecular solid  

3)metallic solid  

4)covalent network solid

Answer:

A- molecular solid

B-metallic solid

C-ionic solid

D-covalent network solid

Explanation:

A molecular solid is held together by weak vanderwaals forces. It can be melted easily but reformed at low temperature when the kinetic energy of molecules is sufficiently reduced. An ionic solid is a network of oppositely charged ions linked together into a three dimensional rigid network. The ions are immobile hence it cannot conduct electricity in the solid state. When the solid melts, the ions become free hence it can now conduct electricity. Metals can be drawn into wire (ductility), this is a fundamental property of metals. Covalent network solid are hard and often have no free valence electrons e.g diamond. They do not conduct electricity

Answer:

C It dictates that the number of atoms of each element must be the same on both sides of a chemical equation.  

Step-by-step explanation:

Atoms have mass, so they can neither be destroyed nor created.

Thus, the number of atoms of each element must be the same on both sides of a balanced chemical equation.  

A is wrong. Molecules consist of different numbers of atoms, and it is atoms that must be conserved.

B is wrong. the Law of conservation of Mass applies to all chemical reactions.

D is wrong. If the reaction proceeds, the mass of reactants must decrease as they are converted to products.

Answer:

The correct answer is option C.

Explanation:

Law of conservation of mass states that mass can neither be created nor be destroyed but it can only be transformed from one form to another form.  

This also means that total mass on the reactant side must be equal to the total mass on the product side that also means the number of atoms of each element must be the same on both sides of a chemical equation.

For example:

[tex]2H_2+O_2\rightarrow 2H_2O[/tex]

Number of hydrogen and oxygen atoms on both sides are equal.

This is false. An alcohol does indeed have a polar C-O single bond, but what we should really be focusing on is the extraordinarily polar O-H single bond. When oxygen, fluorine, or nitrogen is bound to a hydrogen atom, there is a small (but not negligible) charge separation, where the eletronegative N, O, or F has a partial negative charge, and the H has a partial positive charge. Water has two O-H single bonds in it (structure is H-O-H). The partially negative charge on the O of the water molecule (specifically around the lone pair) can become attracted either a neighboring water molecule's partially positive H atom, or an alcohol's partially positive H atom. This is weak (and partially covalent) attraction is called a hydrogen bond. This is stronger than a typical dipole-dipole attraction (as would be seen between neighboring C-O single bonds), and much stronger than dispersion forces (between any two atoms). When the solvent (water) and the solute (the alcohol) both exhibit similar intermolecular forces (hydrogen bonding being the most important in this case), they can mix completely in all proportions (i.e. they are miscible) in water.

Answer:

Explanation:

Took test got it right.

The moles of KClO₃  that were consumed  is  0.343  moles

    calculation

2KClO₃ →  2KCl +3O₂

 step  1: find the  moles    KCl

moles   = mass÷ molar mass

 25.6 g÷74.55 g/mol =0.343  moles

Step 2 : use the  mole  ratio to determine    the  moles  KClO₃

  from  equation above KClO₃ : KCl  is 2:2  =1:1

     therefore   the  moles  KClO₃  = 0.343  moles

Answer: Photoelectric is characterized by or involving the emission of electrons from a surface by the action of light.

Photoelectric effect is the emission of electrons when a radiation of frequency higher than the threshold frequency falls on the surface of an element. The substance which undergoes photoelectric effect is called as photoelectric.

Ground state is the state representing the lowest energy  state.

Excited state is the state which represents a high energy state.

An electron in ground state absorbs energy to move to the excited state.

You might be referring to alkali metals.

Alkali metals are in group 1 of the periodic table.

Alkali metals have a silvery color. Like nearly all main group metals, they reflect light from the entire visible spectrum.

Each of the group 1 atom have one single valence electron. Removing that electron is easy. They are one electron away from the nearest noble gas element. Removing that extra electron will give the atom an empty valence shell. The atom gains stability through that process.

Alkali metals will readily lose its electrons to non-metals such as oxygen, chlorine, and fluorine. They react with water to form a base and hydrogen gas- hence the name alkali. They are too reactive to exist in nature as metals. That's one of the reasons why power packs containing lithium (an alkali metal) should not be cut open at home. They might catch fire when exposed to the air and have a good chance of creating an explosion.

Alkali metals have low m.p. and b.p. among all the metals. They are easy to cut under room temperature. The softness (a.k.a. malleability), melting point, and boiling point of a metal depends on the strength of the bond between its atoms. Each of the group 1 alkali metal atom has one single electron, whereas metals like aluminum have three. Metallic bonds between alkali metal atoms are much weaker than those between aluminum atoms. As a result, it takes less energy to pull alkali metal atoms apart. They are easier to melt, boil, or cut than metals from other groups. For example, it is possible to tear a chunk of sodium but not iron apart by hand.

Alkali metals are likely to be less dense than any other metals on the periodic table. Elements from the same period have an equal number of electron shells. Alkali metals have less protons per atom than elements from the rest of the period. They weakly attract their electron shells and have a large atomic and ionic radius. An alkali metal will have a lofty structure, while metals to the right of the period are more tightly packed.  Alkali metals will have less mass per unit space and have a lower density. For example, typical power banks contain lithium ions rather than nickel. Lithium is lighter than nickel; it allows the battery pack to store more energy per unit mass.

Alkali metals are silvery, soft, highly reactive elements with low melting and boiling points, and are found in Group 1 of the periodic table. These include lithium, sodium, potassium, rubidium, cesium, and francium.

The silvery metals that are soft, highly reactive, and too reactive to be found free in nature, characterized by low melting and boiling temperatures, and low densities, are known as alkali metals. These elements make up Group 1 of the periodic table and include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). Alkali metals react rapidly with water to form hydroxides and hydrogen gas, and they must be stored under oil to prevent reactions with moisture and oxygen from the air.

Their reactivity is due to having one electron in their outermost energy level, which they can easily lose to form positive ions with a charge of +1.

Neutron capture reactions.

Isotopes of the same element have the same number of protons in each nucleus. However, their nucleus differ in the number of neutrons. Adding one or more neutrons to a nucleus will converts it to a different isotope of the same element.

Neutrons can be produced with a particle accelerator. The researcher might aim fast moving alpha particles [tex]\phantom{}_2^{4}\text{He}[/tex] from the accelerator at a beryllium Be target.

[tex]\phantom{}_4^{9} \text{Be} + \phantom{}_2^4\text{He} \to \phantom{}_{\phantom{1}6}^{12}\text{C} + \phantom{}_{0}^{1} \text{n}[/tex]

Doing so will convert beryllium-9 to carbon-12 and release one neutron.

The neutron produced in this process moves very fast ("fast neutrons"). It might knock protons or alpha particles off the target nucleus. This is undesirable since the nucleus will have a change in its proton number. It will end up belonging to a different element.

The researcher should reduce the speed of those neutrons. Passing neutrons through moderators greatly reduces their speed. Moderators are materials that are rich in light nuclei. They remove the energy of neutrons as the two collide. Examples of moderators are heavy water (D₂O) and graphite (carbon). Slow neutrons are easier to capture than fast-moving ones. Combining those slow-moving neutrons to the source isotope will likely produce a different isotope of the same element.

Vitz, Ed. et. al, "19.5: Neutron Bombardment", ChemPRIME (Moore et al.), Libretexts Chemistry, 2017

Answer:

D. BY ADDING OR REMOVING NEUTRONS.

Hope this helps!

Explanation:

Explanation: A thermochemical equation is a balanced chemical equation which require an enthalpy change.

A balanced equation is the equation in which number of atoms on reactant side is same as the number of atoms on product side.

A thermochemical equation for [tex]CaCl_2+H_2O[/tex] is:

[tex]CaCl_2+2H_2O\rightarrow Ca(OH)_2+2HCl+heat[/tex]

Here, heat is released in the reaction hence, it is a type of exothermic reaction.

A thermochemical equation for [tex]NH_4NO_3+H_2O[/tex] is:

[tex]NH_4NO_3+heat\overset{water}{\rightarrow} NH_4^++NO_3^-[/tex]

Here, heat is absorbed in the reaction hence,it is a type of endothermic reaction.

The Cascades rain shadow can be described as such: ocean-influenced moist air masses are forced to rise when they meet the tall moun- tains. The rising air cools, condenses, and the moisture falls as precipitation. On the leeward (dry) side of the mountain, the now dry air warms and sinks.

Answer: The high amount of humidity explains the impressive amount of rain that falls on the Pacific.

Explanation:

In the Pacific Northwest there is a wind current that travels from west to east. It enters the continent and hits a mountain range in a process called "orographic ascent". The jet ascends, the humidity condenses, and the winds coming from the east meet in the opposite direction with this current and push the clouds. That is why the rains are so strong on the Pacific coast. The high amount of humidity explains the impressive amount of rain that falls on the Pacific. When this moist wind blows inland, the moist air may rise into the atmosphere enhancing the clouds and strady rainfall.

Water evaporates from the ocean and is carried over the Northwest , where it cools and condense into the rain.

There is also a low-pressure systems at the surface which is the driving force that produce rain and winds and this allows large storms to crash into the coast with ease. Some of these storms can be enormous and can cause significant wind damage and flooding.

We must to know:

Cm = molarity = niu / Vs, when the niu = no. of moles and Vs = Volume of solution

the no. niu = mass / molecular mass of substance

molecular mass of C8H8 = 12x8+8x1 = 104 g/mol

=> niu = 1,5 / 104 = 0,0144 moles C8H8

=> Cm = 0,0144/0,225 = 0,06 mol/L

Cmm = molality = niu (C8H8) / mass of solvent (kg)

=> p = mass / V => mass (solvent) = p x V

=> 225 x 1,02 = 229,5 g solvent = 0,2295 kg solvent

=> Cmm = 0,0144 / 0,229,5 = 0,063

Answers:

a. 0.064 mol/L; b. 0.063 mol/kg

Explanation:

a. Molar concentration

c = moles/litres

=====

Moles = 1.5 × 1/104.15

Moles = 0.0144 mol

=====

Litres = 225. × 1/1000

Litres = 0.225. L

=====

c = 0.0144/0.225.

c = 0.064 mol·L⁻¹

===============

b. Molal concentration

b = moles of solute/kilograms of solvent

=====

Mass of solvent = 225. × 1.02/1

Mass of solvent = 229.5 g      Convert to kilograms

Mass of solvent = 0.2295 kg

=====

b = 0.0144/0.2295

b = 0.063 mol/kg

Answer: hydrogen atom of a polarized molecule bonds with an electro negative atom.

Explanation:

Hydrogen bonds are special type of dipole dipole forces which are formed when hydrogen bonds with an electro negative element. Hydrogen bonds are strongest type of bonds .Example: Bond between Oxygen of one water molecule to the hydrogen of another water molecule as shown in the image below.

Covalent bonds are formed by sharing of electrons among non metals.

Ionic bond is formed by transfer of electrons between metals and non metals.

The unknown substance that Melinda is encountering in her experiment is most likely a metal, based on its ability to reflect light, warm up in the hand, flatten upon impact, and conduct electricity. These are all characteristic properties of metals.

Based on the properties of the substance highlighted by Melinda - the ability to reflect light, warm up in the hand, flatten out when hit with a hammer, and conduct electricity - it suggests that she is dealing with a metal. These are standard characteristics of metals, which are usually shiny (reflect light), malleable (can be flattened), conductive to heat and electricity, and are known to warm up when handled due to their conductivity.

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