AnswersFL-2003350-Chemistry 1 HonorsReversible Reactions and Equilibrium

Reversible Reactions and Equilibrium Answers

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Consider the reaction below.If the reaction is at dynamic equilibrium at 500 K, which statement applies to the given chemical system?

Question illustration
A
The forward and reverse reactions no longer occur.
B
The rates of the forward and reverse reactions are unequal.
C
The concentrations of the products and reactants do not change.
D
The forward reaction stops at 500 K.
2
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Which represents the correct equilibrium constant expression for the reaction below?

Question illustration
A
K e q equals StartFraction StartBracket upper C u EndBracket StartBracket upper A g superscript plus EndBracket superscript 2 over StartBracket upper C us superscript 2 plus EndBracket StartBracket upper A g EndBracket superscript 2 EndFraction.
Option A
B
K e q equals StartFraction StartBracket upper C u superscript 2 plus EndBracket StartBracket upper A g EndBracket superscript 2 over StartBracket upper C u EndBracket StartBracket upper A g superscript plus EndBracket superscript 2 EndFraction.
Option B
C
K e q equals StartFraction StartBracket upper A g superscript plus EndBracket superscript 2 over StartBracket upper C u superscript 2 plus EndBracket EndFraction.
Option C
D
K e q equals StartFraction StartBracket upper C u superscript 2 plus EndBracket over StartBracket upper A g superscript plus EndBracket superscript 2 EndFraction.
Option D
3

Consider the equilibrium system below.If the system is at dynamic equilibrium, which statement is true?

Question illustration
A
Sublimation of the NH4CI crystals stops.
B
Solidification of the NH4CI vapors stops.
C
The rate of sublimation of the NH4CI crystals is equal to the rate of solidification of the NH4CI vapors.
D
The rate of sublimation of the NH4CI crystals is higher than the rate of solidification of the NH4CI vapors.
4

Consider the reaction.At equilibrium at 600 K, the concentrations are as follows.[HF] = 5.82 x 10-2 M[H2] = 8.4 x 10-3 M[F2] = 8.4 x 10-3 MWhat is the value of Keq for the reaction expressed in scientific notation?

Question illustration
A
2.1 x 10-2
B
2.1 x 102
C
1.2 x 103
D
1.2 x 10-3
5

Which lists all of the substances that appear in equilibrium constant expressions?

A
pure gas and pure liquid
B
pure gas and aqueous solution
C
pure solid and pure liquid
D
aqueous solution and pure liquid
6

The reaction below is at dynamic equilibrium.Which statement is true for the equilibrium system?

Question illustration
A
The concentration of NH3 is greater than the concentration of N2.
B
The concentration of NH3 equals the concentration of N2.
C
The rate of the forward reaction equals the rate of the reverse reaction.
D
The rate of the forward reaction is greater than the rate of the reverse reaction.
7

Which statement correctly describes a reaction in dynamic equilibrium?

A
At dynamic equilibrium, the reactions stop and the amounts of reactants and products do not change.
B
At dynamic equilibrium, the reactions continue but the amounts of reactants and products do not change.
C
At dynamic equilibrium, the reactions stop but the amounts of reactants and products are changing.
D
At dynamic equilibrium, the reactions continue and the amounts of reactants and products are changing.
8

Which statement correctly defines dynamic equilibrium?

A
At dynamic equilibrium, the rates of forward and reverse reactions are equal.
B
At dynamic equilibrium, the rate of the forward reaction is higher than the rate of the reverse reaction.
C
At dynamic equilibrium, the forward and reverse reactions stop.
D
At dynamic equilibrium, the concentrations of reactants and products are equal.
9

Consider the following reversible reaction.What is the equilibrium constant expression for the given system?

Question illustration
A
k subscript e q equals StartFraction StartBracket upper H subscript 2 upper O EndBracket over StartBracket upper H subscript 2 EndBracket StartBracket upper O subscript 2 EndBracket EndFraction.
Option A
B
k subscript e q equals StartFraction StartBracket upper H subscript 2 upper O EndBracket superscript 2 over StartBracket upper H subscript 2 EndBracket superscript 2 StartBracket upper O subscript 2 EndBracket EndFraction.
Option B
C
K subscript e q equals StartFraction StartBracket upper H subscript 2 EndBracket superscript 2 StartBracket upper O subscript 2 EndBracket over StartBracket upper H subscript 2 upper O EndBracket EndFraction.
Option C
D
K subscript e q equals StartFraction StartBracket upper H subscript 2 EndBracket superscript 2 StartBracket upper O subscript 2 EndBracket over StartBracket upper H subscript 2 upper O EndBracket superscript 2 EndFraction.
Option D
10

Consider the reaction.At equilibrium, the concentrations of the different species are as follows.[NH3] = 0.105 M[N2] = 1.1 M[H2] = 1.50 MWhat is the equilibrium constant for the reaction at this temperature?

Question illustration
A
0.0030
B
0.030
C
34
D
340

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