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1. Which quantities are equal in a dynamic equilibrium?
a. the rate constants of the forward and reverse reactions
b. the rates of the forward and reverse reactions
c. the concentrations of the reactants and products
d. the volumes of the reactants and products

2. If the rate constant for the forward reaction in N2O4(g)(colorless) ? 2NO2(g) (brown) is larger than the rate constant forthe reverse reaction, will the constant in [NO2]^2 / [N2O4] =kf/kr
be greater than 1 or smaller than 1?

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Trinidad Tremblay
Trinidad TremblayLv2
21 Apr 2020
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Related questions

Which statement correctly describes a chemical reaction at equilibrium?

1. The concentrations of the products and reactants are equal.

2. The rate of the forward reaction is less than the rate of the reverse reaction.    

3. The rate of the forward reaction is greater than the rate of the reverse reaction.

4. The concentrations of the products and reactants are constant.

4. Consider the following: 2NH3(g) ⇄ N2(g) + 3H2(g)

A flask is initially filled with NH3. As the system approaches equilibrium, the rate of the forward reaction

A. Increases as the rate of the reverse reaction decreases

B. Decreases as the rate of the reverse reaction increases

C. Increases as the rate of the reverse reaction increases

D. Decreases as the rate of the reverse reaction decreases

5. A system at equilibrium is said to be dynamic because at equilibrium the

A. Temperature does not change

B. Macroscopic properties are constant

C. Forward and reverse reactions continue to occur

D. Concentrations of reactants and products are constant

6. In all systems at equilibrium, the

A. Concentration of reactants is less than the concentration of products

B. Concentration of reactants and the concentration of products are equal

C. Concentration of reactants is greater than the concentration of products

D. Concentration of reactants and the concentration of products are constant

Learning Goal:

To understand the relationship between the equilibrium constant and rate constants.

For a general chemical equation

A+B?C+D

the equilibrium constant can be expressed as a ratio of the concentrations:

Kc=[C][D][A][B]

If this is an elementary chemical reaction, then there is a single forward rate and a single reverse rate for this reaction, which can be written as follows:

forward ratereverse rate==kf[A][B]kr[C][D]

where kf and kr are the forward and reverse rate constants, respectively. When equilibrium is reached, the forward and reverse rates are equal:

kf[A][B]=kr[C][D]

Thus, the rate constants are related to the equilibrium constant in the following manner:

Kc=kfkr=[C][D][A][B]

Part A

For a certain reaction, Kc = 7.37

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