Question

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.

          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.

Consider the following reversible reaction:
H2(g) + Cl2(g) 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 (Kc) and calculate the value of Kc at this
temperature. Show all working.
(b) Considering your answer to part (a), does the equilibrium favour reactants or favour products? Justify your
answer.

Added by Ver-Nica M.

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