1/2 N2 (g) +3/2H2 (g) ⇌ NH3 (g) a) Given t=450 C p= 40 atm and...
1/2 N2 (g) +3/2H2 (g) ⇌ NH3 (g)
a) Given t=450 C p= 40 atm and Kp= 7x10^-3 atm^-1 what is Kc?
b) If the gases are placed in a closed reaction vessel with the partial pressures PNH3= 24 atm, PN2= 12 atm and PH2= 36 atm is the system in equilibrium?
c) If the vessel is allowed to expand such that the total pressure is 10 atm will H2 (g) form or be consumed?
d) If the temp is increased from 450C to 1000 C will NH3 be consumed or produced?
Homework Answers
A mixture of gases contains 1.26 g of N2, 3.71 g of H2, and 1.87 g...
A mixture of gases contains 1.26 g of N2, 3.71 g of H2, and 1.87 g of NH3. If the total pressure of the mixture is 1.67 atm, what is the partial pressure of each component? PN2 = ? atm PH2 = ? atm PNH3 = ? atm
A mixture of gases contains 1.26 g of N2, 8.57 g of H2, and 7.28 g...
A mixture of gases contains 1.26 g of N2, 8.57 g of H2, and 7.28 g of NH3. If the total pressure of the mixture is 1.66 atm, what is the partial pressure of each component? PN2 = atm PH2 = atm PNH3 = atm
A mixture of gases contains 8.55 g of N2, 5.51 g of H2, and 1.38 g...
A mixture of gases contains 8.55 g of N2, 5.51 g of H2, and 1.38 g of NH3. If the total pressure of the mixture is 3.07 atm, what is the partial pressure of each component? PN2 = _____ atm PH2 = _____ atm PNH3 = ______atm
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
N2(g) + 3 H2(g) ⇌ 2 NH3(g) KP = 6.78 x 105 at 298 K (determined...
N2(g) + 3 H2(g) ⇌ 2 NH3(g) KP = 6.78 x 105 at 298 K (determined using atm) A 7.5 x 101 L container being held at 298 K is charged with the three gases present in the above equation. Once finished, the initial partial pressure of N2 was 0.59 atm, the initial partial pressure of H2 was 0.45 atm, and the initial partial pressure of NH3 was 0.11 atm. The gas mixture was then allowed to reach equilibrium. Use...
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.
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.
At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches...
At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches equilibrium when the partial pressures of nitrogen, hydrogen, and ammonia gases are 4.00 atm, 1.00 atm, and 1.05 x 10−2 atm, respectively. Given that the standard enthalpy of the reaction at 400K is DH = -94 kJ/mol, estimate the value of the equilibrium constant KP at 450 K assuming that the standard enthalpy of reaction does not vary significantly with temperature in this temperature...
5. A mixture of H2 gas (PH2 2.05 atm), CO2 gas (Pco2 4.10 atm) and water...
5. A mixture of H2 gas (PH2 2.05 atm), CO2 gas (Pco2 4.10 atm) and water vapor (PH20-3.28 atm) are allowed to come to equilibriurm in a closed container. The temperature is 500. K. The equilibrium represented by the equation below is established and the equilibrium partial pressure of H20 is determined to be 3.51 atm. a) Find the equilibrium partial pressures of the CO2, H2, and CO gases. CO2 (g) H2 (g) ←→ CO (g) H2O (g) + +...
3. {7} Consider equilibrium N2 (g) + 3 H2(g) 5 2NH3(g) K, -4,51 x10-at 450 °C....
3. {7} Consider equilibrium N2 (g) + 3 H2(g) 5 2NH3(g) K, -4,51 x10-at 450 °C. For the mixture below indicate the direction of this equilibrium reaction toward product or toward reactants) at the following partial pressures: 105 atm NH3; 35 atm N2; 495 atm H:
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
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.
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.
5. A mixture of H2 gas (PH2 2.05 atm), CO2 gas (Pco2 4.10 atm) and water vapor (PH20-3.28 atm) are allowed to come to equilibriurm in a closed container. The temperature is 500. K. The equilibrium represented by the equation below is established and the equilibrium partial pressure of H20 is determined to be 3.51 atm. a) Find the equilibrium partial pressures of the CO2, H2, and CO gases. CO2 (g) H2 (g) ←→ CO (g) H2O (g) + +...
3. {7} Consider equilibrium N2 (g) + 3 H2(g) 5 2NH3(g) K, -4,51 x10-at 450 °C. For the mixture below indicate the direction of this equilibrium reaction toward product or toward reactants) at the following partial pressures: 105 atm NH3; 35 atm N2; 495 atm H:
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