Consider the following reaction at 298 K: 2H2S (g) + SO2 (g) →3S (s, rhombic) + 2H2O (g),ΔG∘rxn=-102 kJ Is the reaction more or less spontaneous under these conditions than under standard conditions? The reaction is

more spontaneous than under standard conditions.

less spontaneous than under standard conditions.

The reaction is more spontaneous than under standard conditions.

Explanation:

For ΔG°rxn, when it is:

negative: the reaction is spontaneous in the forward direction.

zero: the reaction is at equilibrium.

positive: the reaction is non-spontaneous in the forward direction and spontaneous in the reverse direction.

Since (ΔG°rxn = - 102 kJ) negative value:

So, the reaction is more spontaneous than under standard conditions.