Recall that the rate law only focuses on the reactant concentrations and has a general form of:
Reaction: 2 N2O5 → 4NO2 + O2
Given: 1st order reaction
Rate = 4.82 x 10-3 s-1
[A] = 0.0260 M
The decomposition of N2O5 in carbon tetrachloride proceeds as follows:
2 N2O5 → 4 NO2 + O2
The rate law is first order in N2O5. At 64 oC the rate constant is 4.82 x 10-3 s-1.
What is the rate of reaction when [N2O5] = 0.0260 M?
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