Question

question 15 of 32
what is the equilibrium expression for the reaction below?
c(s) + o₂(g) ⇌ co₂(g)

a. \\(\frac{\text{co}_2}{\text{o}_2}\\)

b. \\(\frac{1}{\text{c}}\\)

c. \\(\frac{\text{co}_2}{\text{o}_2\text{c}}\\)

d. \\(\frac{\text{o}_2\text{c}}{\text{co}_2}\\)

Explanation:

Step1: Recall Equilibrium Expression Rules

For a reaction \( aA + bB
ightleftharpoons cC + dD \), the equilibrium constant expression is \( K = \frac{[C]^c[D]^d}{[A]^a[B]^b} \), where solids (and liquids) are excluded because their concentrations are constant. In the reaction \( \text{C}(s) + \text{O}_2(g)
ightleftharpoons \text{CO}_2(g) \), C is a solid, so we exclude its concentration.

Step2: Apply the Rules to the Reaction

The reactants are \( \text{C}(s) \) (excluded) and \( \text{O}_2(g) \), and the product is \( \text{CO}_2(g) \). Using the equilibrium expression formula, we have \( K = \frac{[\text{CO}_2]}{[\text{O}_2]} \) (since the coefficient of \( \text{O}_2 \) and \( \text{CO}_2 \) is 1, and C is solid so not included).

Answer:

A. \(\frac{[\text{CO}_2]}{[\text{O}_2]}\)