Question 1

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C16H34.How many mL of C16H34 are needed to react with 1.00 mol O2? The density of C16H34 is 0.773 g/mL and its molar mass is 226.43 g/mol.

Accepted Answer

A) 9.23 mL 
B) 12.0 mL 
C) 0.561 mL 
D) 4.61 mL 
E) 0.140 mL

Question 2

Potassium superoxide (KO2, 71.10 g/mol) can be used to generate oxygen gas.If the theoretical yield of O2 (32.00 g/mol) must be 12.0 g, how many grams of KO2 should be used? Assume the reaction occurs in the presence of excess H2O (18.02 g/mol). 
4 KO2(s) + 2 H2O(l)  $\rightarrow$  4 KOH(s) + 3O2 (g)

Accepted Answer

A) 26.7 g 
B) 107 g 
C) 28.1 g 
D) 35.6 g 
E) 20.0 g

Question 3

The combustion of ethanol (CH3CH2OH, 46.7 g/mol) results in the formation of water and carbon dioxide.How many grams of carbon dioxide are produced when 46.1 g of ethanol burns?

Accepted Answer

A) 88.1 g 
B) 44.0 g 
C) 176 g 
D) 22.0 g 
E) 11.0 g

Question 4

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.

Accepted Answer

The answer of Solid nickel(II) phosphate and aqueous sodium chloride...

Question 5

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH₃ and 150 g O₂ react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH₃ (g) + 5O₂ (g) $\rightarrow$ 4 NO(g) +6H₂ O(l)

Accepted Answer

The answer of Nitric oxide (30.01 g/mol) can be produced...

Question 6

Identify the set of stoichiometric coefficients that balance the reaction equation for the combustion of octane. 
C8 H18 (l) +O2 (g) $\rightarrow$ CO2 (g) + H2 O(l)

Accepted Answer

A) 1, 25, 8, 9 
B) 1, 17, 8, 9 
C) 2, 34, 16, 18 
D) 2, 25, 16, 18 
E) None of the above coefficients balance the reaction equation.

Question 7

An iron ore, magnetite, contains only iron and oxygen.In refining 100.0 g of the ore, 72.35 g of iron are obtained.What is the empirical formula of the ore?

Accepted Answer

A) Fe2O3 
B) FeO2 
C) Fe2O5 
D) Fe3O4 
E) FeO

Question 8

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C 16H34.Write the balanced reaction equation for the combustion of C 16H34 and report the sum of the stoichiometric coefficients.

Accepted Answer

A) 117 
B) 120 
C) 76 
D) 83 
E) 4

Question 9

What mass of phosphoric acid (H3PO4, 98.00 g/mol) is produced from the reaction of 10.00 g of P4O10 (283.89 g/mol) with 6.00 g water (18.02 g/mol)?

Accepted Answer

A) 3.45 g 
B) 13.8 g 
C) 21.8 g 
D) 16.0 g 
E) 32.6 g

Question 10

The space shuttle uses liquid hydrogen and liquid oxygen to produce thrust for liftoff in the following reaction: 2H2 (l) +O2 (l) $\rightarrow$2H2 O(g)
If the liquid oxygen supply is set to provide 420 kg/s during a launch, what does the rate of liquid hydrogen supply need to be in kilograms per second?

Accepted Answer

A) 840 kg/s 
B) 210 kg/s 
C) 106 kg/s 
D) 53.1kg/s 
E) 63.4 kg/s

Question 11

A 2.00 g sample of methamphetamine was found to contain 1.61 g C, 0.203 g H, and 0.188 g N.What is its empirical formula?

Accepted Answer

A) C10H15N 
B) C4H6N 
C) C4H9N 
D) C13H20N 
E) C8H10N

Question 12

Suppose the combustion of fossil fuels adds about 8.0 * 1012 kg of carbon to the atmosphere per year in the form of CO2.How much oxygen gas is required to produce this amount of carbon dioxide?

Accepted Answer

A) about 2.1*1013 kg 
B) about 5.8 * 1012 kg 
C) about 4.3 *1012 kg 
D) about 1.1 * 1013 kg 
E) about 4.8 * 1013 kg

Question 13

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

A) 93.7 g 
B) 104 g 
C) 116 g 
D) 150 g 
E) 749 g

Question 14

Extracting copper from sulfide ores can be performed by roasting the ore in oxygen, with a subsequent reaction of copper(I) oxide with carbon.Simplified chemical equations for these steps are shown below.Mathematically combine the two reactions to create an overall balanced equation that contains CU(s) as the only form of copper as a product.Eliminate like terms from your final equation and use the lowest whole-number coefficients possible.Select the statement regarding the overall balanced reaction that is FALSE.
 2 Cu2 S(s) +3O2 (g)  $\rightarrow$  2 Cu2 O(s) + 2 SO2 (g) 
Cu2 O(s) + C(s)  $\rightarrow$  2 Cu(s) + CO(g)

Accepted Answer

A) The balanced reaction requires three moles of oxygen gas. 
B) Two moles of copper result when two moles of carbon react. 
C) Cu2O does not appear in the final balanced equation. 
D) Two moles of CO gas are produced in the overall balanced equation. 
E) There are three reactants and three products in the overall balanced equation.

Question 15

Paris green is a highly toxic emerald green compound with the formula Cu(C2H3O2 )2 . 3Cu(AsO2 )2 .What is its percent by mass arsenic?

Accepted Answer

A) 31.99% 
B) 14.78% 
C) 22.17% 
D) 7.389% 
E) 44.34%

Question 16

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

A) 6.05 kg 
B) 9.07 kg 
C) 18.3 kg 
D) 3.03 kg 
E) 2.00 kg

Question 17

A hydrocarbon is found to be 85.63% C by mass.What is its empirical formula?

Accepted Answer

A) CH 
B) CH2 
C) CH3 
D) C2H 
E) CH4

Question 18

Ibuprofen is 75.69% C, 8.80% H, and 15.51% O by mass.What is its empirical formula?

Accepted Answer

A) C6H9O 
B) C9H9O2 
C) C7H18O2 
D) C7H9O2 
E) C13H18O2

Question 19

Hydroxylamine contains 42.41% N and 9.15% H by mass, with the remainder being oxygen.Determine its empirical formula.

Accepted Answer

A) N14H3O16 
B) N4.6HO5.3 
C) N5HO5 
D) N3H9O 
E) NH3O

Question 20

TiCl₄ (189.68 g/mol), a source of Ti metal, can be produced from titanium dioxide (79.87 g/mol), carbon (12.01 g/mol), and chlorine gas (70.90 g/mol).Identify the limiting reactant if 195 g TiO₂ and 325 g Cl₂ react in the presence of excess C.Assuming 100% yield, calculate the mass of TiCl ₄ produced. 3 Ti O₂ (s) + 4 C(s) + 6 CL₂ (g) $\rightarrow$ 3 Ti CL₄ (s) + 2 CO₂ (g) + 2 CO(g)

Accepted Answer

The answer of TiCl₄ (189.68 g/mol), a source of Ti...

Exam 7: Stoichiometry Mass Relationships and Chemical Reactions

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C₁₆H₃₄.How many mL of C₁₆H₃₄ are needed to react with 1.00 mol O₂? The density of C₁₆H₃₄ is 0.773 g/mL and its molar mass is 226.43 g/mol.

The combustion of ethanol (CH₃CH₂OH, 46.7 g/mol) results in the formation of water and carbon dioxide.How many grams of carbon dioxide are produced when 46.1 g of ethanol burns?

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.

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH₃ and 150 g O₂ react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH₃ (g) + 5O₂ (g) $\rightarrow$ 4 NO(g) +6H₂ O(l)

Identify the set of stoichiometric coefficients that balance the reaction equation for the combustion of octane. C₈ H₁₈ (l) +O₂ (g) $\rightarrow$ CO₂ (g) + H₂ O(l)

An iron ore, magnetite, contains only iron and oxygen.In refining 100.0 g of the ore, 72.35 g of iron are obtained.What is the empirical formula of the ore?

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C ₁₆H₃₄.Write the balanced reaction equation for the combustion of C ₁₆H₃₄ and report the sum of the stoichiometric coefficients.

What mass of phosphoric acid (H₃PO₄, 98.00 g/mol) is produced from the reaction of 10.00 g of P₄O₁₀ (283.89 g/mol) with 6.00 g water (18.02 g/mol) ?

A 2.00 g sample of methamphetamine was found to contain 1.61 g C, 0.203 g H, and 0.188 g N.What is its empirical formula?

Suppose the combustion of fossil fuels adds about 8.0 * 10¹² kg of carbon to the atmosphere per year in the form of CO₂.How much oxygen gas is required to produce this amount of carbon dioxide?

Paris green is a highly toxic emerald green compound with the formula Cu(C₂H₃O₂ ) 2 . 3Cu(AsO₂ ) ₂ .What is its percent by mass arsenic?

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?

A hydrocarbon is found to be 85.63% C by mass.What is its empirical formula?

Ibuprofen is 75.69% C, 8.80% H, and 15.51% O by mass.What is its empirical formula?

Hydroxylamine contains 42.41% N and 9.15% H by mass, with the remainder being oxygen.Determine its empirical formula.

Exam 7: Stoichiometry Mass Relationships and Chemical Reactions

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C16H34.How many mL of C16H34 are needed to react with 1.00 mol O2? The density of C16H34 is 0.773 g/mL and its molar mass is 226.43 g/mol.

The combustion of ethanol (CH3CH2OH, 46.7 g/mol) results in the formation of water and carbon dioxide.How many grams of carbon dioxide are produced when 46.1 g of ethanol burns?

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.

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH3 and 150 g O2 react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH3 (g) + 5O2 (g) →\rightarrow→ 4 NO(g) +6H2 O(l)

Identify the set of stoichiometric coefficients that balance the reaction equation for the combustion of octane. C8 H18 (l) +O2 (g) →\rightarrow→ CO2 (g) + H2 O(l)

An iron ore, magnetite, contains only iron and oxygen.In refining 100.0 g of the ore, 72.35 g of iron are obtained.What is the empirical formula of the ore?

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C 16H34.Write the balanced reaction equation for the combustion of C 16H34 and report the sum of the stoichiometric coefficients.

What mass of phosphoric acid (H3PO4, 98.00 g/mol) is produced from the reaction of 10.00 g of P4O10 (283.89 g/mol) with 6.00 g water (18.02 g/mol) ?

A 2.00 g sample of methamphetamine was found to contain 1.61 g C, 0.203 g H, and 0.188 g N.What is its empirical formula?

Suppose the combustion of fossil fuels adds about 8.0 * 1012 kg of carbon to the atmosphere per year in the form of CO2.How much oxygen gas is required to produce this amount of carbon dioxide?

Paris green is a highly toxic emerald green compound with the formula Cu(C2H3O2 ) 2 . 3Cu(AsO2 ) 2 .What is its percent by mass arsenic?

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?

A hydrocarbon is found to be 85.63% C by mass.What is its empirical formula?

Ibuprofen is 75.69% C, 8.80% H, and 15.51% O by mass.What is its empirical formula?

Hydroxylamine contains 42.41% N and 9.15% H by mass, with the remainder being oxygen.Determine its empirical formula.

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C₁₆H₃₄.How many mL of C₁₆H₃₄ are needed to react with 1.00 mol O₂? The density of C₁₆H₃₄ is 0.773 g/mL and its molar mass is 226.43 g/mol.

The combustion of ethanol (CH₃CH₂OH, 46.7 g/mol) results in the formation of water and carbon dioxide.How many grams of carbon dioxide are produced when 46.1 g of ethanol burns?

Nitric oxide (30.01 g/mol) can be produced from ammonia (17.04 g/mol) and oxygen (32.00 g/mol).Identify the limiting reactant if 75 g NH₃ and 150 g O₂ react.Assuming 100% yield, calculate the mass of excess reactant left over. 4 NH₃ (g) + 5O₂ (g) $\rightarrow$ 4 NO(g) +6H₂ O(l)

Identify the set of stoichiometric coefficients that balance the reaction equation for the combustion of octane. C₈ H₁₈ (l) +O₂ (g) $\rightarrow$ CO₂ (g) + H₂ O(l)

Diesel fuel for automobiles and trucks is a mixture of hydrocarbons that can be modeled by C ₁₆H₃₄.Write the balanced reaction equation for the combustion of C ₁₆H₃₄ and report the sum of the stoichiometric coefficients.

What mass of phosphoric acid (H₃PO₄, 98.00 g/mol) is produced from the reaction of 10.00 g of P₄O₁₀ (283.89 g/mol) with 6.00 g water (18.02 g/mol) ?

Suppose the combustion of fossil fuels adds about 8.0 * 10¹² kg of carbon to the atmosphere per year in the form of CO₂.How much oxygen gas is required to produce this amount of carbon dioxide?

Paris green is a highly toxic emerald green compound with the formula Cu(C₂H₃O₂ ) 2 . 3Cu(AsO₂ ) ₂ .What is its percent by mass arsenic?

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?