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.
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.
