# Stoichiometry- Unit 9: Question Preview (ID: 17506)

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For the reaction SO3 + H2O ® H2SO4, calculate the percent yield if 500. g of sulfur trioxide react with excess water to produce 575 g of sulfuric acid.
a) 82.7%
b) 88.3%
c) 91.2%
d) 93.9%

For the reaction 2Na + Cl2 --- 2NaCl, how many grams of NaCl can be produced from 500. g of chlorine?
a) 112 g
b) 319 g
c) 409 g
d) 825 g

For the reaction Cl2 + 2KBr -- 2KCl + Br2, how many grams of KCl can be produced from 300. g of KBr?
a) 98.7 g
b) 111 g
c) 188 g
d) 451 g

For the reaction HCl + NaOH --- NaCl + H2O, how many moles of HCl are required to produce 150. g of water?
a) 1.50 mol
b) 4.16 mol
c) 8.32 mol
d) 12.2 mol

For the reaction 2H2 + O2 -- 2H2O, how many grams of water are produced from 6.00 mol of hydrogen?
a) 2.00 g
b) 6.00 g
c) 54.0 g
d) 108 g

For the reaction 2Na + 2H2O -- 2NaOH + H2, how many grams of NaOH are produced from 3.0 mol of water?
a) 40. g
b) 80. g
c) 120. g
d) 240. g

Which reactant controls the amount of product formed in a chemical reaction?
a) excess reactant
b) mole ratio
c) composition reactant
d) limiting reactant

For the reaction C + 2H2 -- CH4, how many moles of hydrogen are required to produce 10 mol of methane, CH4?
a) 2 mol
b) 4 mol
c) 10 mol
d) 20 mol

In the equation 2Al2O3  4Al + 3O2, what is the mole ratio of aluminum to oxygen?
a) 10:6
b) 3:4
c) 2:3
d) 4:3

Fewer steps are required to solve stoichiometry problems when
a) the reactant is given in grams and the product is sought in grams.
b) the reactant is given in moles and the product is sought in moles.
c) the reactant is given in grams and the product is sought in liters.
d) the reactant is given in liters and the product is sought in number

In the equation 2KClO3---2KCl + 3O2, how many moles of oxygen are produced when 3.0 mol of KClO3 decompose completely?
a) 1.0 mol
b) 2.5 mol
c) 3.0 mol
d) 4.5 mol

How many mole ratios can be correctly obtained from the chemical equation 2Al2O3(l) --- 4Al(s) + 3O2(g)?
a) 3
b) 4
c) 6
d) 8

To determine the limiting reactant in a chemical reaction involving known masses of the two reactants, which of the following would be most useful?
a) determining the masses of 100 mol of each reactant
b) determining the molar masses of the products
c) calculating bond energies
d) calculating the mass of a single product formed from each reactant

The actual yield of a chemical reaction is generally
a) less than the theoretical yield.
b) greater than the theoretical yield.
c) equal to the percentage yield.
d) greater than the percentage yield.

Actual yield must be determined by
a) experiments.
b) calculations.
c) theoretical yield.
d) estimation.

The coefficients in a chemical equation represent the
a) masses, in grams, of all reactants and products.
b) relative numbers of moles of reactants and products.
c) number of atoms in each compound in a reaction.
d) number of valence electrons involved in the reaction.

A balanced chemical equation allows one to determine the
a) mole ratio of any two substances in the reaction.
b) energy released in the reaction.
c) electron configuration of all elements in the reaction.
d) mechanism involved in the reaction.

For the reaction Cl2 + 2KBr ® 2KCl + Br2, calculate the percent yield if 200. g of chlorine react with excesspotassium bromide to produce 410. g of bromine.
a) 73.4%
b) 82.1%
c) 91.0%
d) 98.9%

What is the mole ratio of H2O to H3PO4 in the following chemical equation?
a) 4 to 6
b) 1 to 6
c) 3 to 2
d) 2 to 3

What is the ratio of the actual yield to the theoretical yield, multiplied by 100%?
a) mole ratio
b) percent yield