Question

The reaction shown below has a negative enthalpy change and a positive entropy change.

Answer 1

Answer:

D. The reaction will be spontaneous at any temperature.

Explanation:

• For the reaction to be spontaneous, the free energy change (ΔG) must be negative (< 0).

∵ ΔG = ΔH - TΔS

where, ΔG is the free energy change.

ΔH is the enthalpy change,

ΔS is the entorpy change.

• Since ΔH is negative and ΔS is positive;

ΔG = (- ve) - T(+ ve) = - ve value.

ΔG will be negative at all temperatures.

So, The reaction will be spontaneous at any temperature.