Equilibrium Questions

1) For the reaction ICl(g) == ½ I₂(g) + ½ Cl₂(g) , K_c = 2.2 x 10^-3 at 25° C. Calculate K_c at this temperature for I₂(g) + Cl₂(g) == 2ICl(g).

2) For the reaction SO₂Cl₂(g) == SO₂(g) + Cl₂(g) , K_c = 0.011 at a particular temperature. A 2.00 L container at this temperature contains 0.30 mole SO₂, 0.20 mole Cl₂, and 0.50 mole SO₂Cl₂.

a) Is this system at equilibrium?

b) If it is not at equilibrium, in which direction will the system move to reach equilibrium? Why?

3) For the reaction SO₂(g) + NO₂(g) == NO(g) + SO₃(g), Kc = 85.0 at 460° C. A reaction is started with 0.0500 M of both reactants ( and no products). Calculate the equilibrium concentration of all species at 460° C.

4) Oxygen dissociates into gaseous atoms according to the equilibrium O₂(g) == 2O(g). At 1800 K the equilibrium constant K_c = 1.2 x 10^-10. One (1.00) mole of O₂ is placed in a 5.0 L flask, heated to 1800 K, and allowed to come to equilibrium at this temperature. Find the equilibrium concentration of all species at 1800 K. (Make a simplifying approximation and check it).

5) Refer to the equilibrium system of Question 3. If an experiment is started with 0.00831 M of both reactants, calculate the equilibrium concentrations of all species at 460 ° C.

ANSWERS