Question

The following homogeneous gaseous equilibrium has an equilibrium constant, Kₚ = 8.37 x 10⁻⁶ at 265 °C. Calculate the Kc value for this reaction.

a) Kc = 8.37 x 10⁻⁶ at 265 °C
b) Kc = 1.20 x 10⁻⁵ at 265 °C
c) Kc = 2.40 x 10⁻¹² at 265 °C
d) Kc = 5.60 x 10⁻³ at 265 °C

Answer 1

To calculate the Kc value from the given Kp value, the balanced chemical equation and change in moles of gas are needed, which are not provided. Therefore, we cannot determine the correct Kc value from the given options.

Step-by-step explanation:

The question asks us to calculate the Kc value for a gaseous equilibrium reaction given the Kp value and temperature. To convert Kp to Kc, we need to use the relationship Kp = Kc(RT)Δn, where R is the universal gas constant, T is the temperature in Kelvin, and Δn is the change in moles of gas. However, to provide a precise answer for the conversion from Kp to Kc, we need the balanced chemical equation to know the value of Δn. Since this information is not provided in the question, we are unable to convert Kp to Kc without further information. Therefore, we cannot answer this question with the options provided a) through d), as each requires additional specific data about the balanced chemical equation.