Question

For a gaseous reaction at 239°C, the equilibrium constant Kc is given as 89.6. Calculate the value of Kp for the same reaction.

A) 20.27
B) 181.4
C) 0.00198
D) 1.12
E) None of the above

For the reaction X(g) + 3Y(g) ⇌ 3Z(g), the equilibrium constant Kp is 1.32×10^(-2) at a temperature of 207°C. Calculate the value of Kc for the same reaction.

A) 0.00135
B) 0.0001
C) 0.01
D) 100
E) None of the above

Answer 1

Without the change in the number of moles of gas and the ideal gas constant R, the conversions between Kc and Kp cannot be completed to provide a correct answer. Additional information is necessary to perform the calculation.

Step-by-step explanation:

To calculate the value of Kp from Kc for a gaseous reaction, we use the equation Kp = Kc(RT)^Δn, where R is the ideal gas constant, T is the temperature in Kelvin, and Δn is the change in the number of moles of gas in the reaction. In the case described, the temperature is given as 239°C, which converts to 512 K. However, we do not have the necessary details about the change in moles of gas (Δn) to calculate Kp, which are crucial for the calculation. As such, none of the options (A to E) can be confirmed as correct without this information.

For the reaction X(g) + 3Y(g) ⇌ 3Z(g), with Kp = 1.32×10-2 at 207°C, we must convert the temperature to Kelvin, which would be 480 K. We can use the equation Kc = Kp / (RT)^Δn to find Kc. The change in the number of moles of gas (Δn) is the number of moles of products minus the number of moles of reactants, which is 3 - (1 + 3) = -1. Again, without further information, such as the value of R used, we cannot calculate Kc from Kp and therefore cannot confirm which of the provided options (A to E) would be correct.