Question

Calculate the reaction quotient (Qc) for the following reaction at 25°C, given the concentration of reactants and products:2NO2(g) + F2(g) ⇌ 2NO2F(g)[NO2] = 0.30 M, [F2] = 0.40 M, [NO2F] = 0.60 M.Is the reaction at equilibrium? If not, in which direction will the reaction proceed to achieve equilibrium?

Answer 1

To calculate the reaction quotient  Qc , we use the expression:Qc = [NO2F]^2 /  [NO2]^2 * [F2] Plugging in the given concentrations:Qc =  0.60 ^2 /   0.30 ^2 *  0.40  Qc = 0.36 /  0.09 * 0.40 Qc = 0.36 / 0.036Qc = 10Now, we need to compare Qc to the equilibrium constant  Kc  to determine if the reaction is at equilibrium or not. However, the value of Kc is not provided in the problem. If Qc > Kc, the reaction will proceed in the reverse direction  toward reactants  to achieve equilibrium.If Qc < Kc, the reaction will proceed in the forward direction  toward products  to achieve equilibrium.If Qc = Kc, the reaction is already at equilibrium.Since we don't have the value of Kc, we cannot determine if the reaction is at equilibrium or in which direction it will proceed to achieve equilibrium.