Question 1

Copper metal reacts with nitric acid to form aqueous copper(II)nitrate,nitrogen monoxide gas,and water.Write the balanced chemical equation.Include states of matter.

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Question 2

Mathematically combine the following three reactions to arrive at the following overall balanced equation for the combustion of the psychostimulant drug methamphetamine (C₁₀H₁₅N).Show your work and write final your equation with whole-number coefficients. (i)C(s)+ O₂(g)$\to$ CO₂(g) (ii)H₂(g)+ O₂(g)$\to$ H₂O (iii)N₂(g)+ 2 O₂(g)$\to$ 2 NO₂(g)

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Question 3

A mass of 11.60 g of phosphoric acid (98.00 g/mol)was produced from the reaction of 10.00 g of P₄O₁₀ (283.9 g/mol)with 12.0 g water (18.02 g/mol).What was the percent yield for this reaction?

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Question 4

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%?

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Question 5

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

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Question 6

If 98.0 g B₂O₃ (69.62 g/mol)and 125 g HF (20.01 g/mol)are combined and allowed to react according to the given equation,what mass of the excess reactant will be left over? B₂O₃(s)+ 6 HF(aq)$\to$ 2 BF₃(g)+ 3 H₂O

Accepted Answer

1 mol B₂O₃ has a mass of 69.62 g. 98.0 g B₂O₃ is equal to 1.41 mol. 1 mol HF has a mass of 20.01 g. 125 g HF is equal to 6.25 mol. According to the balanced chemical equation, 1 mol B₂O₃ reacts with 6 mol HF. The limiting reactant in this case is B₂O₃, as we have only 1.41 mol of it, which is not enough to react with all 6.25 mol HF. Using stoichiometry, we can calculate the amount of HF required to react with all 1.41 mol of B₂O₃: 1 mol B₂O₃ x 6 mol HF/1 mol B₂O₃= 6 mol HF Therefore, the amount of excess HF left over is: 6.25 mol HF - 6 mol HF = 0.25 mol HF Converting this to grams: 0.25 mol HF x 20.01 g/mol = 5.0 g HF To find the mass of excess B₂O₃ left over, we can use stoichiometry again: 1 mol B₂O₃ x 6 mol HF/1 mol B₂O₃= 6 mol HF This means that to react with all 6.25 mol HF, we would need: 6.25 mol HF x 1 mol B₂O₃/6 mol HF = 1.04 mol B₂O₃ Converting this to grams: 1.04 mol B₂O₃ x 69.62 g/mol = 72.3 g B₂O₃ Subtracting the mass of B₂O₃ used from the total mass we started with: 98.0 g - 72.3 g = 25.7 g Therefore, the mass of excess B₂O₃ left over is 25.7 g. The correct answer is B, 25.5 g B₂O₃ will be left over.

Question 7

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

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Question 8

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)+ ______H₂O $\to$______NaAu(CN)₂(aq)+ ______NaOH(aq)

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Question 9

Household bleach contains 5.0% sodium hypochlorite (NaOCl,74.44 g/mol)by mass.Household ammonia contains 5.0% NH₃ (17.04 g/mol)by mass.If they are mixed,toxic chloramine gas (NH₂Cl; 51.48 g/mol)is produced.What volume of NH₂Cl gas results when 50.00 g of bleach and 50.00 g of 5.0% ammonia are combined? Assume 1 mol NH₂Cl occupies 24.4 L. NaOCl(aq)+ NH₃(aq)$\to$ NH₂Cl(aq)+ NaOH(aq)

Accepted Answer

1. Convert mass of NaOCl and NH3 to moles: - Moles of NaOCl = 50.00 g / 74.44 g/mol = 0.672 mol - Moles of NH3 = (5.0/100) x 50.00 g / 17.04 g/mol = 0.147 mol 2. Determine the limiting reagent: - Based on the equation, the stoichiometric ratio between NaOCl and NH3 is 1:1 (1 mol of NaOCl reacts with 1 mol of NH3) - Therefore, NH3 is the limiting reagent because there is less of it than NaOCl 3. Calculate the moles of NH₂Cl produced: - From the equation, 1 mol of NH₂Cl is produced for every 1 mol of NH3 used - Moles of NH₂Cl = 0.147 mol 4. Convert moles of NH₂Cl to volume: - 1 mol of gas occupies 24.4 L - Volume of NH₂Cl produced = 0.147 mol x 24.4 L/mol = 3.59 L = 0.82 L (rounded to 2 significant figures) Therefore, the answer is C.

Question 10

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

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Question 11

A 2.0 kg bottle of sodium carbonate (Na₂CO₃,106.0 g/mol)is available to clean up a 1665 g sulfuric acid spill (H₂SO₄,98.08 g/mol).Is this enough sodium carbonate to neutralize the acid according to the following reaction? H₂SO₄(aq)+ Na₂CO₃(s)$\to$Na₂SO₄(aq)+ CO₂(g)+ H₂O( )

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Question 12

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 copper(II)oxide are produced when 1.00 kg of the copper ore is processed? 2 CuS(s)+ 3 O₂(g)$\to$ 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 13

Quicklime,CaO,can be produced by heating calcium hydroxide,Ca(OH)₂.What is the percent yield if 45 grams of quicklime are obtained from 1 mole of calcium hydroxide?

Accepted Answer

To determine the percent yield, we need to compare the actual yield (45 g) to the theoretical yield of CaO that can be produced from 1 mole of Ca(OH)2.

The balanced equation for the reaction is:
Ca(OH)2 → CaO + H2O

The molar mass of Ca(OH)2 is 74.1 g/mol, and that of CaO is 56.1 g/mol. 
So, 1 mole of Ca(OH)2 produces 1 mole of CaO.

From 1 mole of Ca(OH)2, the theoretical yield of CaO is:
56.1 g/mol x 1 mol = 56.1 g

The percent yield is:
(Actual yield / Theoretical yield) x 100%

= (45 g / 56.1 g) x 100%

= 80%

Therefore, the answer is (B) 80%.

Question 14

Write the balanced reaction equation for the combustion of isooctane (C₈H₁₈),which is found in gasoline.

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Question 15

Calcium hydride (CaH₂,42.10 g/mol)is so reactive with water (18.02 g/mol)that it can be used to remove traces of water from nonaqueous solvents.What mass of the excess reactant will be left over if 24.6 g CaH₂ is added to a large volume of solvent that contains 14.0 g H₂O? CaH₂(s)+ 2H₂O( )$\to$ Ca(OH)₂(s)+ 2H₂(g)

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Question 16

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 17

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?

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Question 18

Nitrogen and oxygen can react to form a number of compounds.If x grams of O₂ combine with y grams of N₂ to form NO₂,how many grams of O₂ combine with y grams of N₂ to make N₂O? Give your answers in terms of x.

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Question 19

Mathematically combine the following three reactions to arrive at the following overall balanced equation for the complete combustion of the tricyclic antidepressant,imipramine (C₁₉H₂₄N₂).Show your work and write your final equation with whole-number coefficients.Assume nitrogen is completely oxidized to NO₂. (i)C(s)+ O₂(g)$\to$ CO₂(g) (ii)H₂(g)+ O₂(g)$\to$H₂O (iii)N₂(g)+ 2 O₂(g)$\to$ 2 NO₂(g)

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Question 20

Nitrogen and oxygen can react to form a number of compounds.If x grams of O₂ combine with y grams of N₂ to form NO,how many grams of O₂ combine with y grams of N₂ to make N₂O? Give your answers in terms of x.

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Quiz 7: Stoichiometry-Mass Relationships and Chemical Reactions

Copper metal reacts with nitric acid to form aqueous copper(II)nitrate,nitrogen monoxide gas,and water.Write the balanced chemical equation.Include states of matter.

A mass of 11.60 g of phosphoric acid (98.00 g/mol) was produced from the reaction of 10.00 g of P₄O₁₀ (283.9 g/mol) with 12.0 g water (18.02 g/mol) .What was the percent yield for this reaction?

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 nitrate into nitrogen gas,oxygen gas,and water vapor.

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

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

Quicklime,CaO,can be produced by heating calcium hydroxide,Ca(OH) ₂.What is the percent yield if 45 grams of quicklime are obtained from 1 mole of calcium hydroxide?

Write the balanced reaction equation for the combustion of isooctane (C₈H₁₈),which is found in gasoline.

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?

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?

Nitrogen and oxygen can react to form a number of compounds.If x grams of O₂ combine with y grams of N₂ to form NO₂,how many grams of O₂ combine with y grams of N₂ to make N₂O? Give your answers in terms of x.

Nitrogen and oxygen can react to form a number of compounds.If x grams of O₂ combine with y grams of N₂ to form NO,how many grams of O₂ combine with y grams of N₂ to make N₂O? Give your answers in terms of x.

Quiz 7: Stoichiometry-Mass Relationships and Chemical Reactions

Copper metal reacts with nitric acid to form aqueous copper(II)nitrate,nitrogen monoxide gas,and water.Write the balanced chemical equation.Include states of matter.

A mass of 11.60 g of phosphoric acid (98.00 g/mol) was produced from the reaction of 10.00 g of P4O10 (283.9 g/mol) with 12.0 g water (18.02 g/mol) .What was the percent yield for this reaction?

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 nitrate into nitrogen gas,oxygen gas,and water vapor.

If 98.0 g B2O3 (69.62 g/mol) and 125 g HF (20.01 g/mol) are combined and allowed to react according to the given equation,what mass of the excess reactant will be left over? B2O3(s) + 6 HF(aq) →\to→ 2 BF3(g) + 3 H2O

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

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)+ ______H2O →\to→ ______NaAu(CN)2(aq)+ ______NaOH(aq)

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

A 2.0 kg bottle of sodium carbonate (Na2CO3,106.0 g/mol) is available to clean up a 1665 g sulfuric acid spill (H2SO4,98.08 g/mol) .Is this enough sodium carbonate to neutralize the acid according to the following reaction? H2SO4(aq) + Na2CO3(s) →\to→ Na2SO4(aq) + CO2(g) + H2O( )

Quicklime,CaO,can be produced by heating calcium hydroxide,Ca(OH) 2.What is the percent yield if 45 grams of quicklime are obtained from 1 mole of calcium hydroxide?

Write the balanced reaction equation for the combustion of isooctane (C8H18),which is found in gasoline.

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?

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?

Nitrogen and oxygen can react to form a number of compounds.If x grams of O2 combine with y grams of N2 to form NO2,how many grams of O2 combine with y grams of N2 to make N2O? Give your answers in terms of x.

Nitrogen and oxygen can react to form a number of compounds.If x grams of O2 combine with y grams of N2 to form NO,how many grams of O2 combine with y grams of N2 to make N2O? Give your answers in terms of x.

A mass of 11.60 g of phosphoric acid (98.00 g/mol) was produced from the reaction of 10.00 g of P₄O₁₀ (283.9 g/mol) with 12.0 g water (18.02 g/mol) .What was the percent yield for this reaction?

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%?

Quicklime,CaO,can be produced by heating calcium hydroxide,Ca(OH) ₂.What is the percent yield if 45 grams of quicklime are obtained from 1 mole of calcium hydroxide?

Write the balanced reaction equation for the combustion of isooctane (C₈H₁₈),which is found in gasoline.

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?

Nitrogen and oxygen can react to form a number of compounds.If x grams of O₂ combine with y grams of N₂ to form NO₂,how many grams of O₂ combine with y grams of N₂ to make N₂O? Give your answers in terms of x.

Nitrogen and oxygen can react to form a number of compounds.If x grams of O₂ combine with y grams of N₂ to form NO,how many grams of O₂ combine with y grams of N₂ to make N₂O? Give your answers in terms of x.