Question

What is the equilibrium constant expression for the following reaction? 2 NO(g) + O2(g) ⇌ 2 NO2(g) Given that the initial concentrations of NO, O2, and NO2 were 0.025 M, 0.015 M, and 0 M, respectively, calculate the equilibrium constant (Kc) at 25°C.

Answer 1

To calculate the equilibrium constant  Kc  for the given reaction, we first need to write the equilibrium constant expression. The equilibrium constant expression for the reaction is:Kc = [NO2]^2 /  [NO]^2 * [O2] Now, we need to find the equilibrium concentrations of each species. Let's denote the change in concentration of each species by x:2 NO g  + O2 g   2 NO2 g -2x      -x         +2xInitial concentrations: 0.025 M  NO , 0.015 M  O2 , and 0 M  NO2 Equilibrium concentrations:  0.025 - 2x  M  NO ,  0.015 - x  M  O2 , and  2x  M  NO2 Now, we can plug the equilibrium concentrations into the Kc expression:Kc = [ 2x ^2] /  [ 0.025 - 2x ^2] * [ 0.015 - x ] Unfortunately, we cannot solve for Kc without additional information, such as the equilibrium concentrations or the initial reaction rate. If you provide that information, we can proceed with the calculation.