Question

Calculate the equilibrium constant Kp for this reaction, given the following information (at 296 K ): 2NO(g)+Br2(g)⇌2NOBr(g)Kc=1.8 2NO(g)⇌N2(g)+O2(g)Kc=2.3×1030

Answer 1

To calculate the equilibrium constant Kp for the reaction given, we can use the given information to convert Kc to Kp and calculate it.

Step-by-step explanation:

To calculate the equilibrium constant Kp for the reaction 2NO(g) + Br2(g) ⇌ 2NOBr(g), we can use the given information:

The equilibrium constant Kc for the reaction 2NO(g) ⇌ N2(g) + O2(g) is 2.3 × 1030.

First, we need to convert the Kc to Kp using the equation Kp = Kc(RT)Δn, where Δn is the difference in moles of gaseous products and gaseous reactants. In this case, Δn = (2+1) - 2 = 1.

Substituting the values into the equation, we get:

Kp = Kc(RT)Δn = (2.3 × 1030)(0.0821)(296)1 = 1.89 × 1032.