chapter 9- Stoichiometry

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

0.903 mol

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

1:2

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

4.5 mol

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

actual yield

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

percent yield

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

theoretical yield

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

1.00 mol

9. For the reaction 2Na + 2H₂O → 2NaOH + H₂, how many grams of sodium hydroxide are produced from 3.0 mol of water?

120 g

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

4:3

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

592 g

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

9.0 mol

What is the percent yield for the reaction Cl₂ + 2KBr → 2KCl + Br₂, in which 200.g of chlorine react with an excess of potassium bromide to produce 410.g of bromine.

90.9%

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

available amount of each reactant.

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

composition stoichiometry

In most chemical reactions the amount of product obtained is

less than the theoretical yield.

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

limiting reactant

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

limiting reactant.

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 to A from the chemical equation.

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

relative numbers of moles of reactants and products.

If the percent yield is equal to 100%, then

the actual yield is equal to the theoretical yield.

You are performing the following reaction in the lab: 2Na + 2H₂0 → 2NaOH + H₂. You are given 120. g of sodium and 80. g of water. What is the limiting reactant? How many grams of H₂ are produced? How many grams of the excess reactant are left over?

water 4.5 g sodium, 19 g