Consider the following reversible reaction:
H2(g) + Cl2(g) \iff 2HCl(g)
(a) In a reaction mixture that is at equilibrium at a certain temperature, the following concentrations were
measured:
[H2] = 0.420 mol L$^{-1}$, [Cl2] = 0.0750 mol L$^{-1}$ and [HCl] = 0.950 mol L$^{-1}$
Write the expression used to calculate the equilibrium constant ($K_c$) and calculate the value of $K_c$ at this
temperature. Show all working.
(b) Considering your answer to part (a), does the equilibrium favour reactants or favour products? Justify your
answer.