Question

1.For the reaction,

PCl₅(g) <-----> PCl₃(g) + Cl₂(g)          K_p = 24.6 at 500 K

calculate the equilibrium partial pressures of the reactants and products if the initial pressures are P_PCl5 = 0.610 atm, P_PCl3 = 0.400 atm and P_Cl2 = 0.000 atm.

P_PCl5 = P_PCl3 = P_Cl2 =

2.

H₂O(g) + Cl₂O(g) <-----> 2HClO(g)          K_c = 0.14 at 298.15 K

calculate the equilibrium concentrations of the reactants and products if the initial concentrations are [H₂O(g)] = 0.00482 mol L^-1, [Cl₂O(g)] = 0.00482 mol L^-1 and [HClO(g)] = 0.000 mol L^-1.

[H₂O(g)] = [ClO₂(g)] = [HClO(g)] =

3.A flask that initially contained pure NO₂ was heated to 1000 K, a temperature at which the value of K_p for the decomposition of NO₂ is 128.8.

2NO₂(g) <-----> 2NO(g) + O₂(g)

Given that the partial pressure of O₂ at equilibrium equals 0.168 atm calculate the partial pressures of NO₂ and NO at equilibrium.

P_NO = P_NO2 =

4.The equilibrium constant K_p for the reaction,

2 SO₃(g) <-------> 2 SO₂(g) + O₂(g)

is 8.440 at 789 °C. If a vessel at this temperature initially contains pure SO₃ and if the partial pressure of SO₃ at equilibrium is 0.050 atm, what is the partial pressure of O₂ in the flask at equilibrium?

What was the initial pressure of SO₃ in the flask?

Answer 1

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