Question

Diatomic and atomic fluorine gas exists in equilibrium according to the following reaction

F2(g) -><- 2F(g)

(a) The standard molar Gibbs free energy of reaction, ∆rG at 298 K is 5.25 kJ mol−1 at 298 K. Use this information to calculate the equilibrium constant for the reaction.

(b) Calculate the extent of reaction, ξ, for this reaction if 1.0 mole of F2 and 0.0 moles of F are present initially. The equilibrium pressure is 1.3 bar.

Answer 1

When 1 mole of reactant is consumed 2 moles of product are formed. This will help you construct ICE Chart. To write the Keqm, you need to know it is the ratio of the product raise to the power of their coefficient divided by the ratio of the reactant raise to the power of its coefficient.

In this first time calculated the mole fraction. The mole fraction was then multiplied with the total pressure to get the partial pressure of the gas. Finally the partial pressures were equated to find the extent of the reaction