# Problem: For the following reaction, ΔH rxn = −120 kJ / mol-rxn and ΔS rxn = −150 J / mol-rxn•K:2NO(g) + O2(g) → 2NO2(g)At what temperatures will this reaction be spontaneous?Note: Remember that we can assume that the ΔH and ΔS values are approximately independent of temperature.Choose 1 answer:a. The reaction is never spontaneous, no matter what the temperature.b. The reaction is spontaneous when T &lt; 800 K.c. The reaction is spontaneous when T &gt; 800 K.d. The reaction is spontaneous at all temperatures.

###### FREE Expert Solution

We are asked for the temperatures at which this reaction would be spontaneous.

First, we look at the Punnet square below to know if we even have to solve or not. ###### Problem Details

For the following reaction, ΔH rxn = −120 kJ / mol-rxn and ΔS rxn = −150 J / mol-rxn•K:

2NO(g) + O2(g) → 2NO2(g)

At what temperatures will this reaction be spontaneous?

Note: Remember that we can assume that the ΔH and ΔS values are approximately independent of temperature.

a. The reaction is never spontaneous, no matter what the temperature.

b. The reaction is spontaneous when T < 800 K.

c. The reaction is spontaneous when T > 800 K.

d. The reaction is spontaneous at all temperatures.