Question 1

Gold metal will dissolve in an aqueous sodium cyanide solution in the presence of O₂. Balance the equation showing this process. ____Au(s)+____ NaCN(aq)+ ____O₂ (g)+ ____H₂ O(l) $\rightarrow$ ___NaAu(CN)₂ (aq)+_____ NaOH(aq)

Accepted Answer

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Question 2

n-Heptane (C₇H₁₆, 00.20 g/mol) is an undesirable component of gasoline because it burns explosively and contributes to engine "knocking." Write the balanced combustion reaction of C ₇H₁₆.Calculate the number of grams of C₇H₁₆ that react if 225 g CO₂ (44.01 g/mol) are produced.

Accepted Answer

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Question 3

Ammonia, NH₃, is industrially produced from N₂ and H₂ using the Haber process.How much ammonia can be produced from 28 kg of nitrogen and 2 kg of hydrogen, assuming the reaction yield is 90%?

Accepted Answer

The balanced chemical equation for the Haber process is:N2 + 3H2 → 2NH3From the equation, we can see that 28 kg of nitrogen will react with 3 * 28 = 84 kg of hydrogen to produce 34 kg of ammonia. However, since the reaction yield is only 90%, the actual amount of ammonia produced will be 34 kg * 0.9 = 30.6 kg. Since 2 kg of hydrogen is used, the limiting reactant is hydrogen, and the maximum amount of ammonia that can be produced is:2 kg H2 * (34 kg NH3 / 84 kg H2) * 0.9 = 9.95 kg NH3Therefore, the correct answer is E) 9.95 kg.

Question 4

Write the balanced reaction equation for the decomposition of solid ammonium perchlorate into nitrogen gas, chlorine gas, oxygen gas, and water vapor.

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Question 5

For which of the following compounds are the empirical and molecular formulas the same? Acetic acid, found in vinegar, CH₃COOH Formaldehyde, used to preserve biological specimens, CH₂O Ethanol, found in beer and wine, CH₃CH₂OH

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Question 6

What is the difference in the chemistry between photosynthesis and respiration? Show the chemical equations for each.Which one releases energy? Which one stores energy?

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Question 7

Carbon emissions by China in 2012 were estimated at approximately 2.6 * 10⁹ metric tons (1 metric ton = 1000 kg).This is equivalent to how many kilograms of CO₂?

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Question 8

Write the balanced reaction equation for the combustion of dodecane (C₁₂H₂₆), which is found in kerosene.

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Question 9

Nicotine is composed of carbon, hydrogen, and nitrogen.A 20.000 g sample was found to contain 14.807 g C and 1.7396 g H.Find the empirical formula of nicotine.

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Question 10

Without doing any calculations, identify which of the following compounds has the largest percent sodium by mass and which has the smallest.Explain your logic. sodium oxide, Na₂O; sodium hydroxide, NaOH; sodium hydrogen carbonate, NaHCO₃; sodium carbonate, Na₂CO₃; sodium peroxide, Na₂O₂

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Question 11

A copper ore consisting of 12.5% copper(II) sulfide 95.61 g/mol), when heated and reacted with oxygen gas 32.00 g/mol), produces copper(II) oxide (79.55 g/mol) and sulfur dioxide (64.06 g/mol).If the reaction has a 90.0% yield, how many grams of copperII) oxide are produced when 1.00 kg of the copper ore is processed? 2 CuS(s) +3 O₂ (g) $\rightarrow$ 2 CuO(s) + 2 SO₂ (g)

Accepted Answer

First, calculate the mass of copper(II) sulfide (CuS) in 1.00 kg of the ore: $1.00 \, \text{kg} \times 12.5\% = 125 \, \text{g}$.The molar mass of CuS is 95.61 g/mol, so the moles of CuS in 125 g are $125 \, \text{g} / 95.61 \, \text{g/mol} = 1.307 \, \text{mol}$.The balanced chemical equation shows that 2 moles of CuS produce 2 moles of CuO. Therefore, 1.307 moles of CuS will produce 1.307 moles of CuO.The molar mass of CuO is 79.55 g/mol, so the mass of CuO produced is $1.307 \, \text{mol} \times 79.55 \, \text{g/mol} = 103.9 \, \text{g}$.Considering the 90.0% yield, the actual mass of CuO produced is $103.9 \, \text{g} \times 90.0\% = 93.51 \, \text{g}$, which rounds to 93.7 g.

Question 12

Calcium carbide (CaC_2, 64.10 g/mol) reacts with water (18.02 g/mol) to produce acetylene gas (C₂H₂, 26.04 g/mol), which is used in welding applications.The other reaction product is calcium hydroxide (Ca(OH)₂, 74.10 g/mol).How many kilograms of C₂H₂ can be produced from 75.0 kg CaC₂?

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Question 13

Fill in the following table regarding the following reaction.
$ \mathrm{UO}_{2}(s)+4 \mathrm{HF}(a q) \rightarrow \mathrm{UF}_{4}(s)+2 \mathrm{H}_{2} \mathrm{O}(\ell) $

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Question 14

Write a definition of the phrase "stoichiometry of a chemical reaction."

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Question 15

In addition to TiS, titanium forms a number of compounds with sulfur.Find the mass percent Ti in TiS, Ti₂S₃, and TiS₂ to two decimal places.

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Question 16

Silver metal reacts with nitric acid to form aqueous silver nitrate nitrate, nitrogen monoxide gas, and water.Write the balanced chemical equation.Include states of matter.

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Question 17

(Na₂B₄O₅OH)₄ . 8 H₂O, commonly known as borax, is used in a variety of applications, including as a fire retardant, an antifungal agent, a flux in metallurgy, a texturing agent in cooking, and a precursor for other boron compounds.How many cubic meters of borax (381.37 g/mol; 1.73 g/cm³) would be required to produce 250 kg elemental boron?

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Question 18

Solid nickel(II) phosphate and aqueous sodium chloride are produced when aqueous solutions of nickel(II) chloride and sodium phosphate are mixed.Write the balanced chemical equation.Include states of matter.

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Question 19

Ammonia (NH₃, 17.04 g/mol) is industrially produced from N₂ and H₂ using the Haber process.What mass of H₂ should be used if 34.0 kg NH₃ must be the final yield when the reaction is run under conditions that produce only a 33.0% yield?

Accepted Answer

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Question 20

Adipic acid is 49.31% C, 6.90% H, and 43.79% O by mass.Find its empirical formula.

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Quiz 7: Stoichiometry Mass Relationships and Chemical Reactions

Gold metal will dissolve in an aqueous sodium cyanide solution in the presence of O₂. Balance the equation showing this process. __Au(s)+ NaCN(aq)+ O₂ (g)+ H₂ O(l) $\rightarrow$ _NaAu(CN)₂ (aq)+_____ NaOH(aq)

n-Heptane (C₇H₁₆, 00.20 g/mol) is an undesirable component of gasoline because it burns explosively and contributes to engine "knocking." Write the balanced combustion reaction of C ₇H₁₆.Calculate the number of grams of C₇H₁₆ that react if 225 g CO₂ (44.01 g/mol) are produced.

Ammonia, NH₃, is industrially produced from N₂ and H₂ using the Haber process.How much ammonia can be produced from 28 kg of nitrogen and 2 kg of hydrogen, assuming the reaction yield is 90%?

Write the balanced reaction equation for the decomposition of solid ammonium perchlorate into nitrogen gas, chlorine gas, oxygen gas, and water vapor.

For which of the following compounds are the empirical and molecular formulas the same? Acetic acid, found in vinegar, CH₃COOH Formaldehyde, used to preserve biological specimens, CH₂O Ethanol, found in beer and wine, CH₃CH₂OH

What is the difference in the chemistry between photosynthesis and respiration? Show the chemical equations for each.Which one releases energy? Which one stores energy?

Carbon emissions by China in 2012 were estimated at approximately 2.6 * 10⁹ metric tons (1 metric ton = 1000 kg).This is equivalent to how many kilograms of CO₂?

Write the balanced reaction equation for the combustion of dodecane (C₁₂H₂₆), which is found in kerosene.

Nicotine is composed of carbon, hydrogen, and nitrogen.A 20.000 g sample was found to contain 14.807 g C and 1.7396 g H.Find the empirical formula of nicotine.

Without doing any calculations, identify which of the following compounds has the largest percent sodium by mass and which has the smallest.Explain your logic. sodium oxide, Na₂O; sodium hydroxide, NaOH; sodium hydrogen carbonate, NaHCO₃; sodium carbonate, Na₂CO₃; sodium peroxide, Na₂O₂

Calcium carbide (CaC_2, 64.10 g/mol) reacts with water (18.02 g/mol) to produce acetylene gas (C₂H₂, 26.04 g/mol), which is used in welding applications.The other reaction product is calcium hydroxide (Ca(OH)₂, 74.10 g/mol).How many kilograms of C₂H₂ can be produced from 75.0 kg CaC₂?

Write a definition of the phrase "stoichiometry of a chemical reaction."

In addition to TiS, titanium forms a number of compounds with sulfur.Find the mass percent Ti in TiS, Ti₂S₃, and TiS₂ to two decimal places.

Silver metal reacts with nitric acid to form aqueous silver nitrate nitrate, nitrogen monoxide gas, and water.Write the balanced chemical equation.Include states of matter.

Solid nickel(II) phosphate and aqueous sodium chloride are produced when aqueous solutions of nickel(II) chloride and sodium phosphate are mixed.Write the balanced chemical equation.Include states of matter.

Ammonia (NH₃, 17.04 g/mol) is industrially produced from N₂ and H₂ using the Haber process.What mass of H₂ should be used if 34.0 kg NH₃ must be the final yield when the reaction is run under conditions that produce only a 33.0% yield?

Adipic acid is 49.31% C, 6.90% H, and 43.79% O by mass.Find its empirical formula.

Quiz 7: Stoichiometry Mass Relationships and Chemical Reactions

Gold metal will dissolve in an aqueous sodium cyanide solution in the presence of O2. Balance the equation showing this process. ____Au(s)+____ NaCN(aq)+ ____O2 (g)+ ____H2 O(l) →\rightarrow→ ___NaAu(CN)2 (aq)+_____ NaOH(aq)

n-Heptane (C7H16, 00.20 g/mol) is an undesirable component of gasoline because it burns explosively and contributes to engine "knocking." Write the balanced combustion reaction of C 7H16.Calculate the number of grams of C7H16 that react if 225 g CO2 (44.01 g/mol) are produced.

Ammonia, NH3, is industrially produced from N2 and H2 using the Haber process.How much ammonia can be produced from 28 kg of nitrogen and 2 kg of hydrogen, assuming the reaction yield is 90%?

Write the balanced reaction equation for the decomposition of solid ammonium perchlorate into nitrogen gas, chlorine gas, oxygen gas, and water vapor.

For which of the following compounds are the empirical and molecular formulas the same? Acetic acid, found in vinegar, CH3COOH Formaldehyde, used to preserve biological specimens, CH2O Ethanol, found in beer and wine, CH3CH2OH

What is the difference in the chemistry between photosynthesis and respiration? Show the chemical equations for each.Which one releases energy? Which one stores energy?

Carbon emissions by China in 2012 were estimated at approximately 2.6 * 109 metric tons (1 metric ton = 1000 kg).This is equivalent to how many kilograms of CO2?

Write the balanced reaction equation for the combustion of dodecane (C12H26), which is found in kerosene.

Nicotine is composed of carbon, hydrogen, and nitrogen.A 20.000 g sample was found to contain 14.807 g C and 1.7396 g H.Find the empirical formula of nicotine.

Without doing any calculations, identify which of the following compounds has the largest percent sodium by mass and which has the smallest.Explain your logic. sodium oxide, Na2O; sodium hydroxide, NaOH; sodium hydrogen carbonate, NaHCO3; sodium carbonate, Na2CO3; sodium peroxide, Na2O2

Calcium carbide (CaC2, 64.10 g/mol) reacts with water (18.02 g/mol) to produce acetylene gas (C2H2, 26.04 g/mol), which is used in welding applications.The other reaction product is calcium hydroxide (Ca(OH)2, 74.10 g/mol).How many kilograms of C2H2 can be produced from 75.0 kg CaC2?

Fill in the following table regarding the following reaction. UO2(s)+4HF(aq)→UF4(s)+2H2O(ℓ) \mathrm{UO}_{2}(s)+4 \mathrm{HF}(a q) \rightarrow \mathrm{UF}_{4}(s)+2 \mathrm{H}_{2} \mathrm{O}(\ell) UO2​(s)+4HF(aq)→UF4​(s)+2H2​O(ℓ)

Write a definition of the phrase "stoichiometry of a chemical reaction."

In addition to TiS, titanium forms a number of compounds with sulfur.Find the mass percent Ti in TiS, Ti2S3, and TiS2 to two decimal places.

Silver metal reacts with nitric acid to form aqueous silver nitrate nitrate, nitrogen monoxide gas, and water.Write the balanced chemical equation.Include states of matter.

Solid nickel(II) phosphate and aqueous sodium chloride are produced when aqueous solutions of nickel(II) chloride and sodium phosphate are mixed.Write the balanced chemical equation.Include states of matter.

Ammonia (NH3, 17.04 g/mol) is industrially produced from N2 and H2 using the Haber process.What mass of H2 should be used if 34.0 kg NH3 must be the final yield when the reaction is run under conditions that produce only a 33.0% yield?

Adipic acid is 49.31% C, 6.90% H, and 43.79% O by mass.Find its empirical formula.

Gold metal will dissolve in an aqueous sodium cyanide solution in the presence of O₂. Balance the equation showing this process. __Au(s)+ NaCN(aq)+ O₂ (g)+ H₂ O(l) $\rightarrow$ _NaAu(CN)₂ (aq)+_____ NaOH(aq)

n-Heptane (C₇H₁₆, 00.20 g/mol) is an undesirable component of gasoline because it burns explosively and contributes to engine "knocking." Write the balanced combustion reaction of C ₇H₁₆.Calculate the number of grams of C₇H₁₆ that react if 225 g CO₂ (44.01 g/mol) are produced.

Ammonia, NH₃, is industrially produced from N₂ and H₂ using the Haber process.How much ammonia can be produced from 28 kg of nitrogen and 2 kg of hydrogen, assuming the reaction yield is 90%?

For which of the following compounds are the empirical and molecular formulas the same? Acetic acid, found in vinegar, CH₃COOH Formaldehyde, used to preserve biological specimens, CH₂O Ethanol, found in beer and wine, CH₃CH₂OH

Carbon emissions by China in 2012 were estimated at approximately 2.6 * 10⁹ metric tons (1 metric ton = 1000 kg).This is equivalent to how many kilograms of CO₂?

Write the balanced reaction equation for the combustion of dodecane (C₁₂H₂₆), which is found in kerosene.

Without doing any calculations, identify which of the following compounds has the largest percent sodium by mass and which has the smallest.Explain your logic. sodium oxide, Na₂O; sodium hydroxide, NaOH; sodium hydrogen carbonate, NaHCO₃; sodium carbonate, Na₂CO₃; sodium peroxide, Na₂O₂

Calcium carbide (CaC_2, 64.10 g/mol) reacts with water (18.02 g/mol) to produce acetylene gas (C₂H₂, 26.04 g/mol), which is used in welding applications.The other reaction product is calcium hydroxide (Ca(OH)₂, 74.10 g/mol).How many kilograms of C₂H₂ can be produced from 75.0 kg CaC₂?

In addition to TiS, titanium forms a number of compounds with sulfur.Find the mass percent Ti in TiS, Ti₂S₃, and TiS₂ to two decimal places.

Ammonia (NH₃, 17.04 g/mol) is industrially produced from N₂ and H₂ using the Haber process.What mass of H₂ should be used if 34.0 kg NH₃ must be the final yield when the reaction is run under conditions that produce only a 33.0% yield?