Chemistry

Chemistry

Problem

For the reaction 2 NO2(g)→2 NO(g)+O2(g)2\,\text{NO}_2(g) \to 2\,\text{NO}(g) + \text{O}_2(g) which of the following correctly relates the instantaneous reaction rates expressed as concentration changes? a) rate=−d[NO2]dt=2 d[NO]dt=2 d[O2]dtrate = -\dfrac{d[\text{NO}_2]}{dt} = 2\,\dfrac{d[\text{NO}]}{dt} = 2\,\dfrac{d[\text{O}_2]}{dt} b) rate=−12 d[NO2]dt=12 d[NO]dt=d[O2]dtrate = -\tfrac{1}{2}\,\dfrac{d[\text{NO}_2]}{dt} = \tfrac{1}{2}\,\dfrac{d[\text{NO}]}{dt} = \dfrac{d[\text{O}_2]}{dt} c) rate=−12 d[NO2]dt=d[NO]dt=12 d[O2]dtrate = -\tfrac{1}{2}\,\dfrac{d[\text{NO}_2]}{dt} = \dfrac{d[\text{NO}]}{dt} = \tfrac{1}{2}\,\dfrac{d[\text{O}_2]}{dt} d) rate=−d[NO2]dt=d[NO]dt=d[O2]dtrate = -\dfrac{d[\text{NO}_2]}{dt} = \dfrac{d[\text{NO}]}{dt} = \dfrac{d[\text{O}_2]}{dt}

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