Problem: The following reaction is first order in N2O5: N2O5(g) → NO3(g) + NO2(g). The rate constant for the reaction at a certain temperature is 0.053/s. What would the rate of the reaction be at [N2O5] = 0.055 M if the reaction were zero order? (Assume the same numerical value for the rate constant with the appropriate units.)

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The following reaction is first order in N2O5: N2O5(g) → NO3(g) + NO2(g). The rate constant for the reaction at a certain temperature is 0.053/s. What would the rate of the reaction be at [N2O5] = 0.055 M if the reaction were zero order? (Assume the same numerical value for the rate constant with the appropriate units.)

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