chem chap 9

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?

0.904 mol

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 mol

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

108 g

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?

120 g

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

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

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

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

4.5 mol

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

6.23 mol

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 mol

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 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

For the reaction represented by the equation SO3 + H2O → H2SO4, calculate the percentage yield if 500. g of sulfur trioxide react with excess water to produce 575 g of sulfuric acid.

93.9

Study of the mass relationships of elements in compounds?

Composition stoichiometry

What is the ratio of the actual yield to the theoretical yield x 100%?

Percent yield

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

Reaction Stoichiometry

Branch of chemistry dealing with the mass relationships of elements in compounds and the mass relationships among reactants and products in chemical reaction

Stoichiometry

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

actual yield

The units of molar mass are

g/mol

In most chemical reactions the amount of product obtained is

less than the theoretical yield

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

limiting reactant

After calculating the amount of reactant B required to completely react with A, then comparing that amount with the amount of B available, one can determine the

limiting reactant

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

limiting reactant

In the chemical reaction represented by the equation wA + xB → yC + zD, a comparison of the number of moles of A to the number of moles of C would be a(n)

mole ratio

A balanced chemical equation allows one to determine the

mole ratio of any 2 substances in the reaction

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

percent yield

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

percentage yield

The coefficients in a chemical equation represent the

relative numbers of moles of reactants and products

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

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

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

theoretical yield