Question

Choose the best answer below. Which of the following reactions will have the largest equilibrium constant at 298 K?
a) 302(g) → 203(9) AGOrxn = +326 kJ
b) Mg(s) + N20(g) → Mgo(s) + N2(g) AG9rxn = -673.0 kJ
c) 2Hg(g) + O2(g) → 2HgO(s) AGºrx = -180.8 kJ
d) CaCO3(s) » Cao(s) + CO2(g) AG = +131.1 kJ
It is not possible to determine the reaction with the largest equilibrium constant using the given information.

Answer 1

Answer:

Explanation:

Relation between ΔG₀ and K ( equilibrium constant ) is as follows .

lnK =  -  ΔG₀ / RT

$K = e^{-\frac{\triangle G_0}{RT}$

The value of R and T are same for all reactions .

So higher the value of negative ΔG₀ , higher will be the value of K  .

Mg(s) + N₂0(g) → MgO(s) + N₂(g)

has the ΔG₀ value of -673 kJ which is highest negative value . So this reaction will have highest value of equilibrium constant K .