객관식
Given the rate law for a reaction is rate = k[NO][O_2]^2 and the initial rate is 0.020 mol L^{-1} s^{-1} when [NO] = 0.10 mol L^{-1} and [O_2] = 0.20 mol L^{-1}, what is the value of the rate constant k at this temperature?
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15. Chemical Kinetics
Rate Law
Multiple Choice
Which of the following is the correct rate law for the elementary reaction: O3(g) + O(g) → 2O2(g)?
A
rate = k[O]
B
rate = k[O3]^2
C
rate = k[O2]^2
D
rate = k[O3][O]
검증된 단계별 안내1
Identify that the reaction given is an elementary reaction, which means the rate law can be written directly from the molecularity of the reaction step.
Write the balanced elementary reaction: \(\mathrm{O_3(g) + O(g) \rightarrow 2O_2(g)}\).
Since the reaction involves one molecule of \(\mathrm{O_3}\) and one atom of \(\mathrm{O}\) colliding, the rate law depends on the concentration of both reactants.
Express the rate law as: \(\text{rate} = k[\mathrm{O_3}][\mathrm{O}]\), where \(k\) is the rate constant.
Confirm that the rate law matches the stoichiometry of the elementary step, and that no other species (like \(\mathrm{O_2}\)) appear in the rate law because they are products, not reactants.
