# Chem equilibrium

1) 1.0 mol hydrogen iodide was heated in a sealed vessel at 700 K and 100 kPa until equilibrium was reached. The equilibrium mixture contained 0.10 mol iodine. Calculate the equilibrium constant, Kp at 700 K for the reaction
2HI (g) H2 (g) I2 (g)

2) 2.0 mol dinitrogen tetroxide were heated at 300 K and 50 kPa in a sealed vessel to equilibrium, which was found to contain 1.4 mol dinitrogen tetroxide. Calculate the equilibrium constant, Kp for the reaction
N2O4 (g) 2NO2 (g)

3) At 60 °C and a total pressure of 105 Pa, dinitrogen tetroxide is 50% dissociated into nitrogen dioxide according to the equation
N2O4 (g) 2NO2 (g)
Calculate a value for the equilibrium constant, Kp, at this temperature.

4) 2.0 mol phosphorus (V) chloride are heated to 523 K in a sealed vessel. The equilibrium mixture at a pressure of 6.72 x 105 Pa contains 1.2 mol chlorine. Calculate the equilibrium constant, Kp, for the reaction
PCl5 (g) PCl3 (g) Cl2 (g) at 523 K

5) 1.0 mol nitrogen and 3.0 mol hydrogen when allowed to come to equilibrium at 650 K and 6.4 x 106; Pa produced a mixture containing 0.8 mol ammonia. Calculate the equilibrium constant, Kp, for the reaction:
N2 (g) 3H2 (g) 2NH3 (g) at 650 K.
(edited 9 months ago)
(edited 9 months ago)
Original post by Roxibox123

1) 1.0 mol hydrogen iodide was heated in a sealed vessel at 700 K and 100 kPa until equilibrium was reached. The equilibrium mixture contained 0.10 mol iodine. Calculate the equilibrium constant, Kp at 700 K for the reaction
2HI (g) H2 (g) I2 (g)

2) 2.0 mol dinitrogen tetroxide were heated at 300 K and 50 kPa in a sealed vessel to equilibrium, which was found to contain 1.4 mol dinitrogen tetroxide. Calculate the equilibrium constant, Kp for the reaction
N2O4 (g) 2NO2 (g)

3) At 60 °C and a total pressure of 105 Pa, dinitrogen tetroxide is 50% dissociated into nitrogen dioxide according to the equation
N2O4 (g) 2NO2 (g)
Calculate a value for the equilibrium constant, Kp, at this temperature.

4) 2.0 mol phosphorus (V) chloride are heated to 523 K in a sealed vessel. The equilibrium mixture at a pressure of 6.72 x 105 Pa contains 1.2 mol chlorine. Calculate the equilibrium constant, Kp, for the reaction
PCl5 (g) PCl3 (g) Cl2 (g) at 523 K

5) 1.0 mol nitrogen and 3.0 mol hydrogen when allowed to come to equilibrium at 650 K and 6.4 x 106; Pa produced a mixture containing 0.8 mol ammonia. Calculate the equilibrium constant, Kp, for the reaction:
N2 (g) 3H2 (g) 2NH3 (g) at 650 K.

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