Study guide chem

In the chemical reaction described by the equation 4Fe(s) + 3O2(g) 2Fe2O3(s), the mole ratio of iron(III) oxide to iron is

1:2.

For the equation P4(s) + 5O2(g) P4O10(s), if 3 mol of phosphorus react with 10 mol of oxygen, the theoretical yield of phosphorus(V) oxide will be

2 mol.

If 6.0 mol of each reactant are available for the above reaction, the mixture remaining after the reaction should contain

2.0 mol As2O3.

Ozone, O3, is produced by the reaction represented by the following equation 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

Ozone, O3, is produced by the reaction represented by the following equation: 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 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 C + 2H2 ® CH4, what is the mole ratio of hydrogen to methane?

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 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

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

3:2

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

4:3

This equation represents a reaction used commercially to produce elemental arsenic by heating arsenic(III) oxide with carbon. If 6.0 mol of each reactant are available for the above reaction, the mixture remaining after the reaction should contain

6.0 mol CO2.

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 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 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 Cl2 + 2KBr ® 2KCl + Br2, calculate the percentage yield if 200. g of chlorine react with excess potassium bromide to produce 410. g of bromine.

91.0%

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%

This equation represents a reaction used commercially to produce elemental arsenic by heating arsenic(III) oxide with carbon. 2As2O3 + 3C 3CO2 + 4As If 6.0 mol of each reactant are available for the above reaction, the mixture remaining after the reaction should contain

?

If, in the reaction A + B C + D, the quantity of B is insufficient to react with all of A,

B is the limiting reactant.

If the percentage yield of I2 is 80% for the following equation, I2O5 + 5CO I2 + 5CO2, then

Neither (a) nor (b)

In the formation of silicon carbide represented by the chemical equation SiO2(s) + 3C(s) SiC(s) + 2CO(g), 8 mol of each reactant are available for the reaction. What substance is the excess reactant?

SiO2(s)

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

actual yield

The measured amount of product obtained from a chemical reaction is the

actual yield.

The units of molar mass are

g/mol.

In the reaction represented by the equation CH4(g) + 2O2(g) CO2(g) + 2H2O(g), a mass of 125 g CH4 is reacted with excess oxygen. The expression is used to calculate the

mass of water produced.

In the reaction represented by the equation CH4(g) + 2O2(g) CO2(g) + 2H2O(g), a mass of 125 g CH4 is reacted with excess oxygen. The expression

mass of water produced.

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 explicitly provides you with the

mole ratios needed to solve a stoichiometry problem.

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

percentage yield

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

percentage yield.

The efficiency of a chemical reaction is best expressed by the

percentage yield.

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

reaction stoichiometry

In stoichiometry, molar mass is used to

relate the mass of a substance to the amount in moles of that substance.

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

In the chemical equation wA + xB yC + zD, if you know the number of moles of A that react, you can determine

the number of moles of each reactant and product.

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

theoretical yield

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

This equation represents a reaction used commercially to produce elemental arsenic by heating arsenic(III) oxide with carbon. 2As2O3 + 3C 3CO2 + 4As If 8.0 mol As2O3 reacts with excess carbon, the theoretical yield of the above reaction is

16 mol As.

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