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 second order? (Assume the same numerical value for the rate constant with the appropriate units.)

FREE Expert Solution

We’re being asked to calculate the rate of the reaction be at [N2O5] = 0.055 M if the reaction were second order. We can calculate the rate constant of the reaction from its rate law.


Recall that the rate law only focuses on the reactant concentrations and has a general form of:

rate law=kAxBy

k = rate constant
A & B = reactants
x & y = reactant orders


Reaction:      N2O5(g) → NO3(g) + NO2(g)

Given:            Order with respect to N2O5(g) = 2

                        Rate constant =0.053 M/s

          

To determine the unit of k, we will use the following equation:

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Problem Details

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 second order? (Assume the same numerical value for the rate constant with the appropriate units.)

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Based on our data, we think this problem is relevant for Professor Zurek's class at UB.