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9 December, 22:17

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.

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Answers (1)
  1. 10 December, 00:47
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    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 t he reaction is spontaneous at high temperatures.
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