Chemistry Chapter 9

Ozone, O3, is produced by the reaction represented by the following equation: NO2(g)+O2(g)=NO(g)+O3(g) What mass of ozone will form from the reaction of 2.0 g of NO2 in a car's exhaust and excess oxygen?

2.1 g O3

For the reaction represented by the equation SO3 + H2O → H2SO4, how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid in an excess of water?

320 g

For the reaction represented by the equation 2Na + 2H2O → 2NaOH + H2, how many grams of hydrogen are produced if 120. g of sodium and 80. g of water are available?

4.5 g

Which equation is not balanced

4H+2O2=4H2O

For the reaction represented by the equation 2Fe + O2→ 2FeO, how many grams of iron(II) oxide are produced from 8.00 mol of iron in an excess of oxygen?

575 g

For the reaction represented by the equation N2 + 3H2→ 2NH3, how many moles of nitrogen are required to produce 18 mol of ammonia

9.0 mol

What is the measured amount of a product obtained from a chemical reaction?

actual yeild

A determination of the masses and number of moles of sulfur and oxygen in the compound sulfur dioxide would be studied in

composition stoichiometry

What is the study of the mass relationships of elements in compounds?

composition stoichiometry

A chemical reaction involving substances A and B stops when B is completely used. B is the

limiting reaction

Which reactant controls the amount of product formed in a chemical reaction?

limiting reaction

If one knows the mass and molar mass of reactant A and the molar mass of product D in a chemical reaction, one can determine the mass of product D produced by using the

mole ratio of D and A from the chemical equation

What is the study of the mass relationships among reactants and products in a chemical reaction?

reaction stoichiometry

Given the equation 3A+2B=2C, the starting mass of A, and its molar mass, and you are asked to determine the moles of C produced, your first step in solving the problem is the multiply the given mass of A by

1 mol A / molar mass A

For the reaction represented by the equation Cl2 + 2KBr → 2KCl + Br2, how many moles of potassium chloride are produced from 119 g of potassium bromide?

1.00 mol

For the reaction represented by the equation 2H2 + O2→ 2H2O, how many grams of water are produced from 6.00 mol of hydrogen?

108g

For the reaction represented by the equation 2H2 + O2→ 2H2O, how many moles of water can be produced from 6.0 mol of oxygen?

12 mol

For the reaction represented by the equation 2Na + 2H2O → 2NaOH + H2, how many grams of sodium hydroxide are produced from 3.0 mol of sodium with an excess of water?

120g

For the reaction represented by the equation Cl2 + 2KBr → 2KCl + Br2, how many grams of potassium chloride can be produced from 300. g each of chlorine and potassium bromide?

188 g

In the reaction represented by the equation N2 + 3H2→ 2NH3, what is the mole ratio of nitrogen to ammonia?

1:2

For the reaction represented by the equation C + 2H2→ CH4, how many moles of hydrogen are required to produce 10 mol of methane, CH4

20 mol

In the reaction represented by the equation N2 + 3H2→ 2NH3, what is the mole ratio of hydrogen to ammonia?

2:1

The Haber process for producing ammonia commercially is represented by the equation N2(g) + 3H2(g) → 2NH3(g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are required?

3.0 Mole

In the equation 2KClO3→ 2KCl + 3O2, how many moles of oxygen are produced when 3.0 mol of KClO3 decompose completely?

4.5 mole

In the reaction represented by the equation 2Al2O3→ 4Al + 3O2, what is the mole ratio of aluminum to oxygen?

4:3

For the reaction represented by the equation 2KlO3→ 2KCl + 3O2, how many moles of potassium chlorate are required to produce 250. g of oxygen?

5.23

For the reaction represented by the equation 2HNO3 + Mg(OH)2→ Mg(NO3)2 + 2H2O, how many grams of magnesium nitrate are produced from 8.00 mol of nitric acid, HNO3, and an excess of Mg(OH)2?

593 g

For the reaction represented by the equation CH4 + 2O2→ CO2 + 2H2O, how many moles of carbon dioxide are produced from the combustion of 100. g of methane?

6.23

For the reaction represented by the equation AgNO3 + NaCl → NaNO3 + AgCl, how many moles of silver chloride, AgCl, are produced from 7.0 mol of silver nitrate AgNO3?

7.0 mol

For the reaction represented by the equation 2Na + Cl2→ 2NaCl, how many grams of chlorine gas are required to react completely with 2.00 mol of sodium?

70.9 g

For the reaction represented by the equation CH4 + 2O2→ 2H2O + CO2, calculate the percentage yield of carbon dioxide if 1000. g of methane react with excess oxygen to produce 2300. g of carbon dioxide.

83.88%

For the reaction represented by the equation Mg + 2HCl → H2 + MgCl2, calculate the percentage yield of magnesium chloride if 100. g of magnesium react with excess hydrochloric acid to yield 330. g of magnesium chloride.

84.2%

When the formula equation Fe3O4+Al=Al2O3 is correctly balanced the coefficient of Fe is number

9

For the reaction represented by the equation Cl2 + 2KBr → 2KCl + Br2, calculate the percentage yield if 200. g of chlorine react with excess potassium bromide to produce 410. g of bromine.

91%

In what kind of reaction do two or more substances combine to form a new compound?

Synthesis reaction

To determine the limiting reactant in a chemical reaction, one must know the

available amount of all reactants

If one knows the mole ratio of a reactant and product in a chemical reaction, one can

calculate the mass of the product produced from a know mass of reactant

To balance a chemical equation, it may be necessary to adjust the

coefficents

A chemist interested in the efficiency of a chemical reaction would calculate the

percent yield

When the limiting reactant in a chemical reaction is completely used, the

reaction stops

A chemical equation is balanced when the

same number of each kind of atom appears in the reactants and in the products

Which branch of chemistry deals with the mass relationships of elements in compounds and the mass relationships among reactants and products in chemical reactions?

stoichiometry

If the percentage yield is equal to 100%, then

the actual yield is equal to the percent yield

Which of the following would not be studied in the branch of chemistry called stoichiometry?

the amount of energy required to break the ionic bonds in calcium flouride

In the chemical equation wA + xB → yC + zD, if one knows the mass of A and the molar masses of A, B, C, and D, one can determine

the mass of any of the reactants or products

Which of the following would be investigated in reaction stoichiometry?

the mass of potassium required to produce a known mass of potassium chloride

What is the maximum possible amount of product obtained in a chemical reaction?

theoretical yield

The units of molar mass are

g/mol

In most chemical reactions the amount of product obtained is

less then the theoretical yield

A balanced chemical equation allows one to determine the

mole ratio of any two substances in the reaction

The coefficients in a chemical equation represent the

number of atoms in each compound in a reaction

What is the ratio of the actual yield to the theoretical yield, multiplied by 100%

percent yeild

To determine the limiting reactant in a chemical reaction involving known masses of A and B, one could first calculate

the number of moles of B and the number of moles of A available

For the reaction represented by the equation Pb(NO3)2 + 2KI → PbI2 + 2KNO3, how many moles of lead(II) iodide are produced from 300. g of potassium iodide and an excess of Pb(NO3)2?

.904 mol

Which coefficients correctly balance the formula NH4NO2=N2+H2O

1,1,2