Question

The equilibrium constant Kc represented by: FeO (s) + CO (g) --> Fe (s) + CO2 (g) at 1000 °C is equal to 0.5. Therefore, the proportion between the number of CO and CO2 molecules, in equilibrium, at this temperature, is: A) 4 CO to 1 CO2 B) 2 CO to 1 CO2 C) 5 CO to 2 CO2 D) 1 CO to 4 CO2 E) 1 CO to 1 CO2

Answer 1

The proportion between the number of CO and CO2 molecules, in equilibrium at 1000 °C, is C) 5 CO to 2 CO2. Thus the correct option is C.

Step-by-step explanation:

The equilibrium constant
`(\(K_c\))` for the given reaction,
`\(FeO (s) + CO (g) \rightarrow Fe (s) + CO_2 (g)\)`, is given as 0.5. The expression for \(K_c\) is determined by the ratio of the concentrations of products to reactants, each raised to the power of their respective coefficients in the balanced equation. In this case, it is expressed as
`\(K_c = ([Fe][CO_2])/([FeO][CO])\).`

To find the ratio of the number of CO to CO2 molecules at equilibrium, we compare the coefficients in the balanced chemical equation. The coefficient of CO is 1, and the coefficient of CO2 is also 1. Therefore, the ratio of CO to CO2 is equal to the ratio of their coefficients in the balanced equation. In this case, it is 5 CO to 2 CO2, corresponding to option C.

This implies that at equilibrium, for every 5 molecules of CO, 2 molecules of CO2 are produced, maintaining the equilibrium constant
`\(K_c\)`at 0.5. Understanding how to interpret and apply the equilibrium constant allows us to deduce the relative concentrations of reactants and products in a chemical reaction at a given temperature.