Chem Test Stoichiometry

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

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 to multiply the given mass of A by.

1 mol A / molar mass A

Which coefficients correctly balance the formula NH4NO2 -> N2 + H2O?

1, 1, 2

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 2H2 + O2 -> 2H2O, how many moles of water can be produced from 6.0 mol 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?

120 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 3Fe + 4H₂O → Fe₃O₄ + 4H₂, how many moles of iron (III) oxide are produced from 500. g of iron in an excess of H₂O?

2.98 mol

For the reaction represented by the equation SO₃ + H₂O → H₂SO₄, how many grams of sulfuric acid can be produced from 200. g of sulfur trioxide and 100. g of water?

245 g

In the reaction represented by the equation C + 2H2 -> CH4, what is the mole ratio of hydrogen to methane?

2:1

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

2:1

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 excess water?

320. 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

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

5.21 mol

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 2Na + Cl₂ → 2NaCl, how many grams of sodium chloride can be produced from 500. g each of sodium and chlorine?

824 g

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%

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

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%

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

Reaction Stoichiometry

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

actual yield

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 known mass of reactant.

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

coefficients.

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

composition stoichiometry.

In most chemical reactions the amount of the 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.

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.

Each of the four types of reaction stoichiometry problems requires using a

mole ratio.

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

mole ratio.

The coefficients in a chemical equation represent the

relative numbers of moles of reactants and products.

If the percentage yield is equal to 100%, then

the actual yield is equal to the theoretical yield.

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