calculate the equilibrium concentrations of n2o4 n 2 o 4 and no2 n o 2 at 25 c c in a vessel tha

Step 1: Calculate the equilibrium concentrations of N2O4 and NO2 using the equilibrium constant

Question

Calculate the equilibrium concentrations of N2O4 and NO2 at 25°C in a vessel that contains an initial N2O4 concentration of 0.0396 M. The equilibrium constant Kc for the reaction N2O4(g) ⇌ 2NO2(g) is 4.64×10^-3 at 25°C. The equilibrium constant Kp for the reaction C(s) + H2O(g) ⇌ CO(g) + H2(g) is 2.44 at 1000 K. The initial partial pressures are PH2O = 1.19 atm, PCO = 1.09 atm, and PH2 = 1.46 atm. Part A: What is the equilibrium partial pressure of H2O? Express your answer with the appropriate units. Part B: What is the equilibrium partial pressure of CO? Phosphine (PH3) decomposes at elevated temperatures, yielding gaseous P2 and H2: 2PH3(g) ⇌ P2(g) + 3H2(g) with Kp = 398 at 873 K. Part A: If the initial partial pressures are PPH3 = 0.0270 atm, PP2 = 0.863 atm, PH2 = 0.512 atm, calculate Qp. Gaseous indium dihydride is formed from the elements at elevated temperature: In(g) + H2(g) ⇌ InH2(g) with Kp = 1.48 at 973 K. Partial pressures measured in a reaction vessel are: PIn = 0.0650 atm, PH2 = 0.0300 atm, PInH2 = 0.0750 atm. Part A: Calculate Qp. Part B: Determine the direction of reaction to attain equilibrium. Part C: Determine the equilibrium partial pressure of In. Part D: Determine the equilibrium partial pressure of H2. Part E: Determine the equilibrium partial pressure of InH2.

          Calculate the equilibrium concentrations of N2O4 and NO2 at 25°C in a vessel that contains an initial N2O4 concentration of 0.0396 M. The equilibrium constant Kc for the reaction N2O4(g) ⇌ 2NO2(g) is 4.64×10^-3 at 25°C.

The equilibrium constant Kp for the reaction C(s) + H2O(g) ⇌ CO(g) + H2(g) is 2.44 at 1000 K. The initial partial pressures are PH2O = 1.19 atm, PCO = 1.09 atm, and PH2 = 1.46 atm.

Part A:
What is the equilibrium partial pressure of H2O?
Express your answer with the appropriate units.

Part B:
What is the equilibrium partial pressure of CO?
Phosphine (PH3) decomposes at elevated temperatures, yielding gaseous P2 and H2:
2PH3(g) ⇌ P2(g) + 3H2(g) with Kp = 398 at 873 K.

Part A:
If the initial partial pressures are PPH3 = 0.0270 atm, PP2 = 0.863 atm, PH2 = 0.512 atm, calculate Qp.

Gaseous indium dihydride is formed from the elements at elevated temperature:
In(g) + H2(g) ⇌ InH2(g) with Kp = 1.48 at 973 K.
Partial pressures measured in a reaction vessel are: PIn = 0.0650 atm, PH2 = 0.0300 atm, PInH2 = 0.0750 atm.

Part A:
Calculate Qp.

Part B:
Determine the direction of reaction to attain equilibrium.

Part C:
Determine the equilibrium partial pressure of In.

Part D:
Determine the equilibrium partial pressure of H2.

Part E:
Determine the equilibrium partial pressure of InH2.

Added by Anthony G.

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