Equilibrium help

Question

the reactions for 1 and 2 below, take place at 20°C, and answer the following questions.

1) H​2S​ O​3(​ g) ⟶ SO​2(​ g) + H​2​O(g) △Go​ ​ = +25kJ mol-​ 1

2) H​2(​ g) + Cl​2(​ g) ⟶ 2 HCl(g) △Go​ ​ = -400 kJ mol-​1

For each reaction, 1 and 2 calculate the equilibrium constant, ​K​, and is the equilibrium position lying to the right or the left.

∆​G​° = –​RT​ ln ​K​ where ​R​ = 8.31 J mol-​ 1​ K-​ 1​

and ​T​ / K = 273 + ​T​ / °C

which direction will each reaction shift when there is an increase of pressure?

Calculate the reaction quotient for reaction 1 under the following conditions: 25C(degree celcius); [SO​2]​ =0.01M; [H​2O​ ]=0.04M; [H​2​SO​3]​ =0.01M. In which direction will the reaction lie.

Answer 1

1) K = [SO₂][H₂O]/[H₂SO₃]

∆G = =RT lnK

25,000 J/mole = -8.31 J/mol-K x 293K lnK

lnK = 25,000/-2435

lnK = -10.27

K = 3.4x10^-5

An increase in pressure will shift the react to the left (toward reactants) because there are 2 moles of gas on the product side and only one mole of gas on the reactant side.

2) Do same type calculations as above.

An increase in pressure will shift the reaction to the right (product side) because there are 2 moles of gas on the reactant side and only 1 mole of gas on the product side.

Q = [SO2][H2O]/[H2SO3] = (0.01)(0.04)/(0.01) = 0.04

Q is > K so equilibrium lies to the right