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d. The value of Kp for the reaction represented below is 8.3 x 10-3 at 700K. NH3(g) + H2S(g) → NH4HS(g) Calculate the value of Kp at 700K for each of the reactions represented below i) NH4HS(g) →→→ NH3(g) + H2S(g) ii) 2 H2S(g) + 2NH3(g) → 2 NH4HS(g)

d. The value of Kp for the reaction represented below is 8.3 x 10-3 at 700K. NH3(g) + H2S(g) → NH4HS(g) Calculate the value of Kp at 700K for each of the reactions represented below i) NH4HS(g) →→→ NH3(g) + H2S(g) ii) 2 H2S(g) + 2NH3(g) → 2 NH4HS(g)

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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d. The value of Kp for the reaction represented below is 8.3 × 10-3 at 700K. NH3(g) + H2S(g) → NH4HS(g) Calculate the value of Kp at 700K for each of the reactions represented below i) NH4HS(g) → NH3(g) + H2S(g) ii) 2 H₂S(g) + 2NH3(g) → 2 NH4HS(g)
Transcribed Image Text:d. The value of Kp for the reaction represented below is 8.3 × 10-3 at 700K. NH3(g) + H2S(g) → NH4HS(g) Calculate the value of Kp at 700K for each of the reactions represented below i) NH4HS(g) → NH3(g) + H2S(g) ii) 2 H₂S(g) + 2NH3(g) → 2 NH4HS(g)
4. For the reaction represented below, the value of the equilibrium constant at 700K is 3.1 X 10-4. N2(g) + 3 H₂(g) →2 NH3(g) a. Write the expression for the equilibrium constant, Kp, for the reaction b. Assume that the initial partial pressures of the gases are as follows: P(N2) = 0.711 atm, P(H2) = 0.303 atm, and P(NH3) = 0.524 atm. i) Calculate the value of the reaction quotient, Q, at these initial conditions ii) Predict the direction in which the reaction will proceed at 700K if the initial partial pressures are those given above. Justify your answer
Transcribed Image Text:4. For the reaction represented below, the value of the equilibrium constant at 700K is 3.1 X 10-4. N2(g) + 3 H₂(g) →2 NH3(g) a. Write the expression for the equilibrium constant, Kp, for the reaction b. Assume that the initial partial pressures of the gases are as follows: P(N2) = 0.711 atm, P(H2) = 0.303 atm, and P(NH3) = 0.524 atm. i) Calculate the value of the reaction quotient, Q, at these initial conditions ii) Predict the direction in which the reaction will proceed at 700K if the initial partial pressures are those given above. Justify your answer
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