Question

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

203 (g) yields 3O2 (g)

Which of the following best describes this reaction? (1 point)

A. The reaction will only be spontaneous at high temperatures.
B. The reaction will only be spontaneous at low temperatures.
C. The reaction will not be spontaneous at any temperature.
D. The reaction will be spontaneous at any temperature.

Answer 1

D. The reaction will be spontaneous at any temperature.

Step-by-step 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.