The equilibrium constant, K, for the Haber reaction is 2.81 x 10^-5 at 472 C, if a reaction STARTS with 3 bar of H2, and 5 bar of N2 at 472 C, what is the equilibrium pressure of NH3? be sure to justify whether or not any assumptions made the calculations appropriate.
N2 (g) + 3 H2 (g) == 3NH3 (g)
The equilibrium constant, K, for the Haber reaction is 2.81 x 10^-5 at 472 C, if...
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 Haber process for the production of ammonia involves the equilibrium N2(g) + 3 H2(g) ⇌ 2 NH3(g) Assume that Δ H° = -92.38 kJ and ΔS° = -198.3 J/K for this reaction do not change with temperature. a. Without doing calculations, predict the direction in which ΔG° for the reaction changes with increasing temperature. Explain your prediction. b. Calculate ΔG° at 25 °C and 500 °C. c. At what temperature does the Haber ammonia process become nonspontaneous? d. Calculate...
In a series of equilibrium, haber and their collaborations mixed hydrogen and nitrogen in a vessel, and let it reach equilibrium at 472 C. The equilibrium mixture contained 0.1207 M H2, 0.0402 M N2, and 0.00272 M NH3. From this information, calculate the equilibrium constant.
For the following reaction, the equilibrium constant is 3.9 X 10s at 300. K and 0.12 at 500. K. Calculate ??? and ?So for this reaction. N2(g) +3 H2(g) 2 NH3(g)
3. Consider the ammonia production reaction, N2(g)+3H2(g) = 2NH3 (g) The equi librium constant for this reaction at 298K is 6.10x 105. When the system starts with 2 mol of NH3 (no H2 or N2), it reaches the equilibrium at the total pressure of 2.0 bar (a) What is the mole fraction of each species at equilibrium? (b) If we increase the total pressure to 3.0 bar, will it be stimulating the decompo- sition of ammonia? Explain
12) The equilibrium constant, Kp, is 4.51x10 at 450°C for the reaction represented below. N2(g) + 3 H2(g) 2 NH3(g) a. Write the equilibrium expression, Kp, for the reaction. b.Suppose y ou start out with only reactants in a rigid container. The initial partial pressure of N2(g) is 1.0 atm and that of H2(g) is 1.4 atm. What are the partial pressures of each species when the system reaches equilibrium? c. Find K, for this process at 450°C.
What is the equilibrium constant of the formation reaction of ammonia gas at 298.15 K under the conditions that the partial pressures of N2, H2 and NH3 are 2.00 bar, 3.00 bar, and 2.00 bar, respectively? (Hint: Be careful! This is a trick question! The equilibrium constant is what it is. It is not dependent on what the partial pressures happen to be at any particular time. K is purely dependent on the standard Gibbs free energy of the reaction..)
1 pts D Question 8 The Haber process for the production of ammonia is the main industrial process of producing ammonia today. Prior to developing this process, ammonia was difficult to produce on an industrial scale. The reaction for the Haber process is: N2(g)+ 3 H2(8) 2 NH3(g). Using the following values, determine the equilibrium constant for this reaction at 25°C. AG(KJ/mol) Substance N2 H2 NH3 -16.4 Enter your answer to three significant figures.
1.A) What is the equilibrium constant for a reaction at temperature 31.5 °C if the equilibrium constant at 55.4 °C is 1.53? For this reaction, ΔrH = 20.2 kJ mol-1 . You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". 1B) What is the ΔrG° for the following reaction (in kJ mol-1)? N2(g) + O2(g) + Cl2(g)...
Nitrogen and hydrogen react to produce ammonia (Haber process). the Kp for the reaction is 4.51 x 10^-5 at 450 degrees C. determine if the following mixtures are at equilibrium at 450 degrees C. If not, indicate the direction (toward product or toward reactants) in which the mixture must shift to achieve equilibrium. (Calculate Qp for each case). N2 (g) + 3H2 (g) ⇌ 2 NH3 (g) a) 98 atm Nh3, 45 atm N2, 55 atm H2 b) 57 atm...