HomeworkLib
Question

The equilibrium constant, K, for the Haber reaction is 2.81 x 10^-5 at 472 C, if...

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)

science   biology   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
The equilibrium constant, K, for the Haber reaction is 2.81 x 10^-5 at 472 C, if...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • Which is the correct equilibrium constant (K expression) for Haber process? N2 (g) + 3 H2...

    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) ⇌...

    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,...

    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...

    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 298...

    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) +...

    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...

    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..)

  • A) For the Haber process, N2(g) + 3H2(g) <---> 2NH3(g), Kp = 4.34 x 10–3 at...

    A) For the Haber process, N2(g) + 3H2(g) <---> 2NH3(g), Kp = 4.34 x 10–3 at 300oC. Pure NH3 is placed in a 2.00 L flask and is allowed to reach equilibrium at 300oC. There are 3.00 g NH3 in the equilibrium mixture. Calculate the mass (in g) of H2 in the equilibrium mixture. B) The value of Kc for the reaction is 1.2 . The reaction is started with [H2 ]0 = 0.76 M, [N2]0 = 0.60 M and...

  • 1 pts D Question 8 The Haber process for the production of ammonia is the main...

    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...

    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)...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT