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Presuming each of the following overall reactions has the same relative enthalpy for the system, which of the overall reactions shows a process with a change in Gibbs free energy value at constant temperature?


$ NO_{2(g)} + NO_{2(g)} \rightarrow NO_{3(g)} + NO_{(g)}$
$ NO_{3(g)} + CO_{(g)} \rightarrow NO_{2(g)} + CO_{2(g)}$


$ O_{3(g)} \rightarrow O_{2(g)} + O_{(g)}$
$ O_{3(g)} + O_{(g)} \rightarrow 2O_{2(g)}$


$ Cl_{(g)} + O_{3(g)} \rightarrow ClO_{(g)} + O_{2(g)}$
$ ClO_{(g)} + O_{(g)} \rightarrow Cl_{(g)} + O_{2(g)}$


$ NO_{(g)} + Br_{2(l)} \rightarrow NOBr_{2(g)}$
$ NO_{(g)} + NOBr_{2(g)} \rightarrow 2NOBr_{(g)}$

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