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?
Homework Answers
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 = [](http://img.homeworklib.com/questions/aed4e120-ded0-11eb-bd7b-578fe2d01a25.png?x-oss-process=image/resize,w_560)
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For: N2(g) + 3H2(g) ⬄ 2NH3(g), Kp = 4.72 x 10–4 at 475 oC. At
equilibrium...
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.
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...
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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...
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The equilibrium constant, K. for the following reaction is 2.20x104 at 723K 2NH3(8) N2(g) + 3H2(8)...
The equilibrium constant, K. for the following reaction is 2.20x104 at 723K 2NH3(8) N2(g) + 3H2(8) If an equilibrium mixture of the three gases in a 13.1 L container at 723K contains NH, at a pressure of 0.693 atm and Ny at a pressure of 1.02 atm, the equilibrium partial pressure of His atm. Submit Answer Retry Entire Group 9 more group attempts remaining
8. (3 points) Consider the following reaction: N2 (g) +3H2 (g) 2NH3 (g). Find the desired...
8. (3 points) Consider the following reaction: N2 (g) +3H2 (g) 2NH3 (g). Find the desired values given the following conditions: PNH3 2.00 atm, PN2 2.00 atm, and PH2 -2.50 atm. The AGo -33.3 kJ/mol at 25 °C. Calculate the Q value for these conditions. a. b. Calculate the AG value for these conditions. c. Is the reactions more or less spontaneous under these conditions compared to the standard conditions? How do you know?
The equilibrium constant for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is Kp=0.111 at 231 ∘C. Calculate the value...
The equilibrium constant for the chemical equation N2(g)+3H2(g)−⇀↽−2NH3(g) is Kp=0.111 at 231 ∘C. Calculate the value of Kc for the reaction at 231 ∘C.
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) 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.
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...
The equilibrium constant, K. for the following reaction is 2.20x104 at 723K 2NH3(8) N2(g) + 3H2(8) If an equilibrium mixture of the three gases in a 13.1 L container at 723K contains NH, at a pressure of 0.693 atm and Ny at a pressure of 1.02 atm, the equilibrium partial pressure of His atm. Submit Answer Retry Entire Group 9 more group attempts remaining
8. (3 points) Consider the following reaction: N2 (g) +3H2 (g) 2NH3 (g). Find the desired values given the following conditions: PNH3 2.00 atm, PN2 2.00 atm, and PH2 -2.50 atm. The AGo -33.3 kJ/mol at 25 °C. Calculate the Q value for these conditions. a. b. Calculate the AG value for these conditions. c. Is the reactions more or less spontaneous under these conditions compared to the standard conditions? How do you know?
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