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What is the equilibrium expression for the reaction below?

[tex]\[ C (s) + O_2 (g) \rightleftarrows CO_2 (g) \][/tex]

A. [tex]\(\frac{\left[ O_2 \right] [ C ]}{\left[ CO_2 \right]}\)[/tex]

B. [tex]\(\frac{1}{[C]}\)[/tex]

C. [tex]\(\frac{\left[ CO_2 \right]}{\left[ O_2 \right] [ C ]}\)[/tex]

D. [tex]\(\frac{\left[ CO_2 \right]}{\left[ O_2 \right]}\)[/tex]

Sagot :

GinnyAnswer
To determine the equilibrium expression for the given reaction:
[tex]\[ C (s) + O_2 (g) \rightleftarrows CO_2 (g) \][/tex]

we need to follow these steps:

1. Identify the states of matter:
- Carbon (C) is a solid.
- Oxygen (O_2) is a gas.
- Carbon dioxide (CO_2) is a gas.

2. Understand the equilibrium expression:
For a general reaction:
[tex]\[ aA + bB \rightleftarrows cC + dD \][/tex]
the equilibrium expression [tex]\( K \)[/tex] is given by:
[tex]\[ K = \frac{[C]^c [D]^d}{[A]^a [B]^b} \][/tex]
where the square brackets [ ] denote the concentration of the species.

3. Exclude solids and pure liquids:
In the equilibrium expression, we exclude solids and pure liquids because their activities are constant and taken as 1. In this reaction, carbon (C) is a solid and will not appear in the equilibrium expression.

4. Write the equilibrium expression:
For the reaction:
[tex]\[ C (s) + O_2 (g) \rightleftarrows CO_2 (g) \][/tex]
the equilibrium expression involves only the gases:
[tex]\[ K = \frac{[CO_2]}{[O_2]} \][/tex]

Given the choices:
A. [tex]\( \frac{[O_2] [C]}{[CO_2]} \)[/tex]
B. [tex]\( \frac{1}{[C]} \)[/tex]
C. [tex]\( \frac{[CO_2]}{[O_2] [C]} \)[/tex]
D. [tex]\( \frac{[CO_2]}{[O_2]} \)[/tex]

The correct equilibrium expression is:
[tex]\[ \frac{[CO_2]}{[O_2]} \][/tex]

Thus, the answer is :

D. [tex]\( \frac{[CO_2]}{[O_2]} \)[/tex]
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