Which is the correct equilibrium constant (K expression) for Haber process? N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) ΔH = –46.19 kJ
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Which is the correct equilibrium constant (K expression) for Haber process? N2 (g) + 3 H2...
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...
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...
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.
The Haber-Bosch process is used to make ammonia from nitrogen and hydrogen: N2(g) + 3 H2(g) 2 NH3(g). A 10.0 L reactor at 450 °C is filled with 3 moles of nitrogen and 12 moles of hydrogen, K is 0.16 under these conditions.
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)
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.
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.
The synthesis of ammonia by the Haber process occurs by the reaction 3 H2(g)= 2 NH3(g) AH° and AS N2(g) at 400 °C.Using data from Appendix D and essentially unchanged in the temperature interval from assuming that are 25 to 400 °C, estimate Kat 400 °C
The synthesis of ammonia by the Haber process occurs by the reaction 3 H2(g)= 2 NH3(g) AH° and AS N2(g) at 400 °C.Using data from Appendix D and essentially unchanged in the temperature interval...