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Question

Is the question formulated correctly? If not, please correct it. Here is the question: 'Consider the reaction: 2 NO( g) + O2( g) → 2 NO2( g). Estimate ΔG° for this reaction at each temperature and predict whether or not the reaction is spontaneous, assuming that ΔH° and ΔS° do not change significantly within the given temperature range. a. 298 K b. 855 K.'

Accepted Answer

Identify the given reaction: $2 \text{NO}(g) + \text{O}_2(g) \rightarrow 2 \text{NO}_2(g)$.. Understand that you need to estimate $\Delta G^\circ$ for the reaction at two different temperatures: 298 K and 855 K.. Recall the Gibbs free energy equation: $\Delta G^\circ = \Delta H^\circ - T\Delta S^\circ$, where $T$ is the temperature in Kelvin.. Assume that $\Delta H^\circ$ and $\Delta S^\circ$ are constant over the temperature range. You will need these values to calculate $\Delta G^\circ$ at each temperature.. Calculate $\Delta G^\circ$ for each temperature using the equation and determine the spontaneity of the reaction: if $\Delta G^\circ < 0$, the reaction is spontaneous; if $\Delta G^\circ > 0$, it is non-spontaneous.