HomeworkLib
Question

For: N2(g) + 3H2(g) ⬄ 2NH3(g), Kp = 4.72 x 10–4 at 475 oC. At equilibrium...

For: N2(g) + 3H2(g) ⬄ 2NH3(g), Kp = 4.72 x 10–4 at 475 oC. At equilibrium at 475 oC, PH2 = 0.237 atm and PN2 = 0.582 atm. What is the partial pressure of ammonia at equilibrium?

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

Homework Answers

Answer #1

Partial pressure of ammonia = 1.91*10-3 atm

N₂(g) + 3H₂(g) ² 2NH₂ (9) PN = 0.582 atm Pa = 0.237 am Kp = 4.728104 Given At equilibrium к: LPo»,1* [PM] [PH] = 4.72x10 = [

0 0
Add a comment
Know the answer?
Add Answer to:
For: N2(g) + 3H2(g) ⬄ 2NH3(g), Kp = 4.72 x 10–4 at 475 oC. At equilibrium...
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

  • KP = 1.000 x 10–4 for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). The reaction is...

    KP = 1.000 x 10–4 for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g). The reaction is at equilibrium when PH2 = 4.00 atm, PN2 = 4.00 atm, and PNH3 = 0.16 atm. a) Show that these are equilibrium concentrations. b) If the pressure of the system is doubled (the pressure of each gas doubles), what is the final pressure of each gas when equilibrium is restored? If making and using ammonia is important to feeding the world's growing population but...

  • HQ14.35 Unanswered The reaction mixture N2(g) +3H2(g)2NH3(g) has the following equilibrium partial pressures: PN2- 2.40 atm,...

    HQ14.35 Unanswered The reaction mixture N2(g) +3H2(g)2NH3(g) has the following equilibrium partial pressures: PN2- 2.40 atm, PH2-1.60 atm, and PNH3 22.10 atm. Calculate the equilibrium constant Kp. Report your answer to the correct number of significant figures. Type your response

  • AGº is -32.7 kJ/mol of N2 for the reaction N2 (g) + 3H2 (g) = 2NH3(g)...

    AGº is -32.7 kJ/mol of N2 for the reaction N2 (g) + 3H2 (g) = 2NH3(g) This calculation was for the reaction under standard conditions—that is, with all gases present at a partial pressure of 1 atm and a temperature of 25°C. Calculate AG for the same reaction under the following nonstandard conditions: . PN2 = 2.00 atm, PH2 = 7.00 atm, PNH3 = 0.021 atm, . and T = 100°C.

  • Calculate the equilibrium equilibrium constant Kp for the reaction: N2 + 3H2 ↔ 2NH3, if the...

    Calculate the equilibrium equilibrium constant Kp for the reaction: N2 + 3H2 ↔ 2NH3, if the partial pressures of N2, H2, and NH3 are 1.20 atm, 1.97 atm, and 0.225 atm  respectively. A. 0.055 B. 0.532 C. 0.952 D. 18.2

  • Consider the following reaction where Kp = 4.55×10-5 at 723 K: N2(g) + 3H2(g) 2NH3(g) If...

    Consider the following reaction where Kp = 4.55×10-5 at 723 K: N2(g) + 3H2(g) 2NH3(g) If the three gases are mixed in a rigid container at 723 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: 1. A reaction will occur in which NH3(g) is consumed. 2. Kp will increase. 3. A reaction will occur in which N2 is consumed. 4. Q...

  • 2. At 55°C, the equilibrium constant for the reaction N2(g) + 3H2(g) + 2NH3(g) is Kp=0.05....

    2. At 55°C, the equilibrium constant for the reaction N2(g) + 3H2(g) + 2NH3(g) is Kp=0.05. What is the equilibrium constants Kc and Kp for the reaction 4NH3 + 2N2(g) + 6H2(g)? Kp = 400 Kc = 7.62 x 10 3. For the reaction given below, 10.00 moles of A and 25.00 moles of B are placed in a 5.00-L container at 120 °C. A(g) +2B(g) → C(g) At equilibrium, the concentration of A is 0.5 mol/L. What is the...

  • 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...

  • At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP...

    At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP = 7.16. If the initial pressure of NO is 0.00663 atm, what are the equilibrium partial pressures of NO, N2, and O2? p(NO) = . p(N2) = . p(O2) = .

  • The equilibrium constant, Kp, is 4.51 x 10-35 at 450c for the reaction expressed below. N2...

    The equilibrium constant, Kp, is 4.51 x 10-35 at 450c for the reaction expressed below. N2 (g) + 3H2 (g) equilibrium arrows 2 NH3 (g) a. Write the equilibrium expression for, Kp, for the reaction. b. Supposed you start out with only reactants in a rigid container. The initial partial pressure of N2 (g) is 1 atm and that of H2 is 1.4 atm. What ate the partial pressure of each species when the system reaches equilibrium? Can you explain...

  • Consider this reaction: N2(g) + 3H2(g) <==> 2NH3(g) If the Kc for the reaction is 4.5...

    Consider this reaction: N2(g) + 3H2(g) <==> 2NH3(g) If the Kc for the reaction is 4.5 x 10^4 at 127 degrees celsius, what is the equilibrium constant, Kp at the same temperature?

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