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Part A
Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ
Calculate ΔG°rxn for the following reaction. 18 NO(g) → 6 N2O(g) + 6 NO2(g)
Answer Choices To Choose From: A) -3.83 kJ B) -138 kJ C) -23.0 kJ D) 23.0 kJ E) 138 kJ
Part B
CO2(g)→C(s)+O2(g)ΔH∘rxn= +393.5 kJ
(ΔSsys<0, ΔSsurr<0)
In addition, predict under what temperatures (all temperatures, low temperatures, or high temperatures), if any, the reaction in part D will be spontaneous
A) The reaction is spontaneous at all temperatures.
C) The reaction is spontaneous at high temperatures.
D) The reaction is nonspontaneous at all temperatures.

Respuesta :

The correct answer for the question that is being presented above is this one: "C) The reaction is spontaneous at high temperatures." 
Since dH is positive and dS ~ 0 then -TdS ~ 0, meaning dG will always be greater than 0 so the reaction is spontaneous at high temperatures.

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