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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
electron configuration of all elements in the reaction.
B
energy released in the reaction.
C
mechanism involved 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 atoms in each compound in a reaction.
C
number of valence electrons involved in the reaction.
D
relative numbers of moles of reactants and products.
3) Actual yield must be determined by
A
experiments.
B
theoretical yield.
C
calculations.
D
estimation.
4) The actual yield of a chemical reaction is generally
A
equal to the percentage yield.
B
less than the theoretical yield.
C
greater than the theoretical yield.
D
greater than the percentage 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
6
B
8
C
3
D
4
7) 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
3.0 mol
C
4.5 mol
D
2.5 mol
8) In the equation 2Al2O3 4Al + 3O2, what is the mole ratio of aluminum to oxygen?
A
3:4
B
2:3
C
10:6
D
4:3
9) 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 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 moles and the product is sought in moles.
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
2 mol
C
4 mol
D
20 mol
11) Which reactant controls the amount of product formed in a chemical reaction?
A
excess reactant
B
mole ratio
C
composition reactant
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
240. g
B
40. g
C
120. g
D
80. g
14) For the reaction HCl + NaOH --- NaCl + H2O, how many moles of HCl are required to produce 150. g of water?
A
8.32 mol
B
4.16 mol
C
1.50 mol
D
12.2 mol
15) 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
451 g
D
188 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
409 g
C
112 g
D
319 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
91.2%
B
88.3%
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
82.1%
B
73.4%
C
98.9%
D
91.0%
19) What is the mole ratio of H2O to H3PO4 in the following chemical equation?
A
3 to 2
B
2 to 3
C
4 to 6
D
1 to 6
20) What is the ratio of the actual yield to the theoretical yield, multiplied by 100%?
A
percent yield
B
mole ratio
C
Avogadro yield
D
excess yield
*select an answer for all questions
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