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Stoichiometry- Unit 9
Test Description: Stoichiometry- Unit 9
Instructions: Answer all questions to get your test result.
1) A balanced chemical equation allows one to determine the
A
mechanism involved in the reaction.
B
energy released in the reaction.
C
electron configuration of all elements in the reaction.
D
mole ratio of any two substances in the reaction.
2) The coefficients in a chemical equation represent the
A
masses, in grams, of all reactants and products.
B
number of valence electrons involved in the reaction.
C
number of atoms in each compound in a reaction.
D
relative numbers of moles of reactants and products.
3) Actual yield must be determined by
A
experiments.
B
theoretical yield.
C
estimation.
D
calculations.
4) The actual yield of a chemical reaction is generally
A
equal to the percentage yield.
B
greater than the theoretical yield.
C
greater than the percentage yield.
D
less than the theoretical yield.
5) 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
calculating bond energies
C
determining the molar masses of the products
D
calculating the mass of a single product formed from each reactant
6) 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
7) In the equation 2KClO3---2KCl + 3O2, how many moles of oxygen are produced when 3.0 mol of KClO3 decompose completely?
A
3.0 mol
B
2.5 mol
C
1.0 mol
D
4.5 mol
8) In the equation 2Al2O3 4Al + 3O2, what is the mole ratio of aluminum to oxygen?
A
4:3
B
3:4
C
10:6
D
2:3
9) Fewer steps are required to solve stoichiometry problems when
A
the reactant is given in moles and the product is sought in moles.
B
the reactant is given in grams and the product is sought in liters.
C
the reactant is given in liters and the product is sought in number
D
the reactant is given in grams and the product is sought in grams.
10) For the reaction C + 2H2 -- CH4, how many moles of hydrogen are required to produce 10 mol of methane, CH4?
A
10 mol
B
20 mol
C
2 mol
D
4 mol
11) Which reactant controls the amount of product formed in a chemical reaction?
A
excess reactant
B
composition reactant
C
mole ratio
D
limiting reactant
12) For the reaction 2H2 + O2 -- 2H2O, how many grams of water are produced from 6.00 mol of hydrogen?
A
2.00 g
B
108 g
C
6.00 g
D
54.0 g
13) For the reaction 2Na + 2H2O -- 2NaOH + H2, how many grams of NaOH are produced from 3.0 mol of water?
A
80. g
B
120. g
C
40. g
D
240. g
14) 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
12.2 mol
C
4.16 mol
D
8.32 mol
15) For the reaction Cl2 + 2KBr -- 2KCl + Br2, how many grams of KCl can be produced from 300. g of KBr?
A
111 g
B
451 g
C
188 g
D
98.7 g
16) For the reaction 2Na + Cl2 --- 2NaCl, how many grams of NaCl can be produced from 500. g of chlorine?
A
825 g
B
319 g
C
112 g
D
409 g
17) 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
88.3%
B
91.2%
C
93.9%
D
82.7%
18) 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
91.0%
B
98.9%
C
82.1%
D
73.4%
19) What is the mole ratio of H2O to H3PO4 in the following chemical equation?
A
3 to 2
B
4 to 6
C
1 to 6
D
2 to 3
20) What is the ratio of the actual yield to the theoretical yield, multiplied by 100%?
A
Avogadro yield
B
excess yield
C
percent yield
D
mole ratio
*select an answer for all questions
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