For the equilibrium, 2 NOCl (g) 2 NO (g)+ Cl ₂(g) , the value of the equilibrium constant, K_ C is 3.75 10⁻⁶ at 1069 ~K . The value of K_ p for the reaction at this temperature will be

Step-by-step solution

The relationship between the equilibrium constants K_ p and K_ c is given by the equation K_ p = K_ c (RT)^ n_ g . For the reaction 2 NOCl (g) 2 NO (g) + Cl ₂(g) , the change in the number of moles of gaseous species is calculated as n_ g = (2 + 1) - 2 = 1 . Given values are K_ c = 3.75 10⁻⁶ , R = 0.0821 L atm K ⁻¹ mol ⁻¹ , and T = 1069 K . Substituting these values into the formula: K_ p = (3.75 10⁻⁶) (0.0821 1069)¹ K_ p = 3.75 10⁻⁶ 87.7649 K_ p 0.000329118 Rounding to the appropriate precision, K_ p 0.00033 . Ans