Calculate the equilibrium constant for the following reaction at 100°C.

Question

2 TiCl3(g)+2 HCl (g) = 2 TiCl4(g)+H2(g)
∆G°rxn = + 47.0 kJ mol-1

cant i just use K = e^ -Delta G/RT? --> K = e ^ -47.0 kJ mol-1 /(8.314)(273+100)?
what is the point of having the balanced equation?

or am i not supposed to use that formula at all

Answer 1

The way I see it is that you have a reaction that is dGo = 47.0 kJ/mol and you have two moles which makes it 94 kJ for the reaction as written.