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13) For the reaction: 2N2O5(g) ?4NO2(g) +O2(g) the rate law is: ?[O2] ?t = k[N2O5] At 300 K, the half-life is 2.50
For the reaction:2N2O5(g) ? 4NO2(g) + O2(g)d[N2O5]/dt = -1.9Ã10-2 M/s at a particular temperature and set ofconcentrations.What are d[O2]/dt and d[NO2]/dt?d[O2]/dt =d[NO2]/dt =What is the rate of the reaction?For the reaction:4NO2(g) + O2(g) ? 2N2O5(g)d[O2]/dt = -2.1Ã10-2 M/s at a particular temperature and set ofconcentrations.What are d[NO2]/dt and d[N2O5]/dt?d[NO2]/dt =d[N2O5]/dt =What is the rate of the reaction?
For the following reaction if the rate of disappearance of O2 is0.0450 mol L-1s-1, what is the rate of formation N2O5(g)?4NO2(g) + O2(g)---> 2N2O5(g)