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
Step 1. Calculate the order of the reaction with respect to N2O5.
Use experimental data 1 and 2 (you can use any):
x = order
(Larger concentration should be on the numerator)
Solve for x:
since the numerator and the denominator are raised to the same power, you can simplify the equation to:
2.53 raised to the power of 1 = 2.53
x = 1 → 1st order with respect to N2O5
Step 2. Determine the rate law of the reaction
Substitute N2O5 and O2 and their orders:
rate law = k[N2O5]1
rate = k[N2O5]
Step 3. Calculate the value of the rate constant
The following data were obtained for the gas‑phase decomposition of dinitrogen pentoxide,
2 N2O5 (g) → 4 NO2 (g) + O2 (g)
Defining the rate as -Δ[N2O5] / Δt, write the rate law and calculate the value of the rate constant.
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.