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.Calculate the rate of the reaction when [N2O5] = 5.6×10−2 M .

🤓 Based on our data, we think this question is relevant for Professor Hoffman & Ilies' class at DREXEL.

FREE Expert Solution

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:      N2O(g) → NO(g) + NO2 (g)

Given:            Order with respect to N2O5 = 1

                        Rate constant (k) = 0.053 s-1

                        [N2O5] = 0.056 M

Calculate for the rate constant, k:

View Complete Written Solution
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.

Calculate the rate of the reaction when [N2O5] = 5.6×10−2 M .

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Rate Law concept. You can view video lessons to learn Rate Law. Or if you need more Rate Law practice, you can also practice Rate Law practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Hoffman & Ilies' class at DREXEL.