A P Chemistry Test
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4A P Chemistry
Chapter 13 Pre-Test
____ 1. Indicate the mass action expression for the following reaction:
2
3
[ ] [ ]
X Y
[ ] [ ]
W V
[
3
W V
][ ]
3
2
[
2
X Y
][ ]
[ ] [ ]
W V
[ ] [ ]
X Y
A)
B)
C)
D) [X]
[Y][W]
[V]
2
3
____ 2. The value of the equilibrium constant, K, is dependent on
I. The temperature of the system.
II. The nature of the reactants and products.
III. The concentration of the reactants.
IV. The concentration of the products.
A) I, II
B) II, III
C) III, IV
D) It is dependent on three of the above choices.
E) It is not dependent on any of the above choices.
____ 3. Apply the law of mass action to determine the equilibrium expression for
A) [NO
Cl]
[NO
]
[Cl
]
D) 2[NO
Cl]/2[NO
][Cl
]
2
2
2
2
2
2
2
2
B) 2[NO
][Cl
]/2[NO
Cl]
E) [NO
Cl]
/[NO
]
[Cl
]
2
2
2
2
2
2
2
2
C) [NO
]
[Cl
]/[NO
Cl]
2
2
2
2
2
Use the following to answer questions 4-5:
Consider the chemical system
K = 4.6 × 10
L/mol.
9
____ 4. If the concentration of the product were to double, what would happen to the equilibrium
constant?
A) It would double its value.
B) It would quadruple its value.
C) It would not change its value.
D) It would depend on the initial conditions of the product.
E) It would become half its current value.
____ 5. Determine the equilibrium constant for the system
at 25°C. The
] = 4.27 × 10
] = 1.41 × 10
concentrations are shown here: [N
O
M, [NO
M
–2
–2
2
4
2
A) 0.66 B) 3.0 C) 0.0047 D) 0.33 E) 0.05
____ 6. Consider the reaction
whose K = 54.8 at 425°C. If an equimolar mixture of
reactants gives the concentration of the product to be 0.50 M at equilibrium, determine the
concentration of the hydrogen.
A) 1.6 × 10
M B) 4.6 × 10
M C) 9.6 × 10
M D) 6.8 × 10
M E) 1.2 × 10
M
–4
–3
–2
–2
–3
March 8, 2001 Page 1
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