Using the equilibrium constant expression given below, calculate the equilibrium constant if [N2] = 0.063 M, [H2] = 9.2 × 10−3 M, and [NH3] = 1.8 × 10−4 M. Enter your answer in the provided box. Keq = [NH3]2 [N2][H2]3
Using the equilibrium constant expression given below, calculate the equilibrium constant if [N2] = 0.063 M,...
Using the equilibrium constant expression given below, calculate the equilibrium constant if (N2) = 0.061 M, H2] =9.1 x 10M , and (NH3 1 = 1.8 X 10 M. Enter your answer in the provided box. Keg [NH] [N2][12] Keg
Using the equilibrium constant expression Keq = [NH3]2/ [N2][H2]3 and the equilibrium constant of Keq = 0.586, determine the equilibrium concentration of NH3 if the concentration of N2 is 5.4 × 10−2 M, and the concentration of H2 is 5.4 × 10−3 M. Enter your answer in the provided box.
Using the equilibrium constant expression Keq = [NH3]^2 / [N2][H2]^3 and the equilibrium constant of Keq = 0.586, determine the equilibrium concentration of NH3 if the concentration of N2 is 6.0 × 10−2 M, and the concentration of H2 is 5.0 × 10−3 M. Enter your answer in the provided box.
Using the equilibrium constant expression Keq = [NH3]2 [N2][H2]3 and the equilibrium constant of Keq = 0.586, determine the equilibrium concentration of NH3 if the concentration of N2 is 5.4 × 10−2 M, and the concentration of H2 is 2.7 × 10−3 M. Enter your answer in the provided box.
Using the equation shown below, calculate the equilibrium concentration of N2 given that the equilibrium concentration of H2 is 2.0 M and the equilibrium concentration of NH3 is 0.5 M. For the reaction at this temperature, Kc = 2. N2(g) + 3 H2(g) ⇌ 2 NH3(g)
Which is the correct equilibrium constant (K expression) for Haber process? N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) ΔH = –46.19 kJ A. A) K = [P]/[R] = [NH3]/[N2][H2] B. B) K = [P]/[R] = [NH3]2/[N2][H2]3 C. C) K = [P]/[R] = [NH3]2/[H2]3 D. D) K = [P]/[R] = [NH3]/[N2][H2]3 E. E) none of the above
the equilibrium constant is given for two of the reactions below. Determine the value of the missing 23) - equilibrium constant A(g) +B(g) - AB(g) AB(g) + A(g) - A2B(g) 2 A(g) +B(g) - A2B(g) Ke=0.24 Ke = 3.8 Ke=? A) 0.63 B) 4.0 C) 16 D) 0.91 E) 3.6 24) 24) Determine the value of Kp for the following reaction, at 300K, if the equilibrium concentrations are as follows: (N2leq -1.5M, [H2leq = 1.1 M, (NH3 leq = 0.47...
Enter your answer in the provided box. A reaction vessel contains NH3, N2, and H, at equilibrium at a certain temperature. The equilibrium concentrations are [N21 -0.66 M, [12= 1.16 M, and (NH31 -0.70 M. Calculate the equilibrium constant, K, if the reaction is represented as H2(g) = NH3(g)
The equilibrium constant K for the reaction N2 + 3H22NH, is 0.159 at 450°C. Calculate the equilibrium composition when 2.50 mol N2 is mixed with 7.50 mol H2 in a 5.00 L vessel. [N] - M [H2] M (NH3) M Submit Answer Try Another Version 6 Item attempts remaining
A reaction vessel contains NH3, N2, and H2 at equilibrium at a certain temperature. The equilibrium concentrations are [N2] = 0.61 M, [H2] = 1.26 M, and [NH3] = 0.30 M. Calculate the equilibrium constant, Kc, if the reaction is represented as ( 1 2 ) N2(g) + ( 3 2 ) H2(g) ⇌ NH3(g)