🤓 Based on our data, we think this question is relevant for Professor Hoffman & Ilies' class at DREXEL.
Recall that the rate law only focuses on the reactant concentrations and has a general form of:
k = rate constant
A & B = reactants
x & y = reactant orders
Reaction: N2O5 (g) → NO3 (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:
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 .
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Based on our data, we think this problem is relevant for Professor Hoffman & Ilies' class at DREXEL.