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 equilibrium constant expression Keq = [NH3]2 [N2][H2]3 and the equilibrium constant of Keq =...
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 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) = 0.061 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
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
Consider the reaction: N2(g) + 3 H2(g) « 2 NH3(g) a. Write the expression for the equilibrium constant, K, for this reaction. b. An equilibrium misture of N2, H2, and NH3 at 300°C is analyzed, and it is found that: [N2] = 0.25 mol/L, [H2] = 0.15 mo/L, and [NH3] = 0.090 mol/L. Find K at 300°C for this reaction.
For the reaction N2(g) + 3 H2(g) equilibrium reaction arrow 2 NH3(g) at 25.0°C, the Kc of the reaction is 5.4 ✕ 105. Use the given concentrations to determine the following. [N2] = 0.0028 M [H2] = 0.0045 M [NH3] = 0.30 M (a) Determine Q at this time. (Omit units.)
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)
1. Write the equilibrium constant expression for the reaction N2 (g) + 3 H2 (g) D 2 NH3 (g) 2. For the reaction in question 1, delta H = -92 kj*mol^-1 Predict the direction of shift of the equilibrium of the above reaction caused by adding N2 at constant volume and temperature removing H2 at constant volume and temperature adding N2 at constant volume and temperature raising the temperature at constant total pressure 3. Hydrogen fluoride (HF) is a weak...
9. What does it mean if Keq < 1, at equilibrium? The concentration of reactants is greater than the concentration of products. b. The concentration of products is greater than the concentration of reactants. The rate of the forward reaction is greater than the rate of the reverse reaction. c. d. The rate of the reverse reaction is greater than the rate of the forward reaction. e. The concentration of products and reactants are about the same. Which of the...