Multiple Choice
Based on the given two-step mechanism for the formation of 2NO2(g) from NO(g) and O2(g), what is the rate law for the overall reaction?
15. Chemical Kinetics
Rate Law
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Using the figure, calculate the value of the rate constant, k, for the reaction. Express your answer using two significant figures.
A
0.12 M^-1s^-1
B
0.25 M^-1s^-1
C
0.50 M^-1s^-1
D
1.00 M^-1s^-1
Verified step by step guidance1
Identify the order of the reaction from the given figure or data. This will help determine the units of the rate constant, k.
Use the rate law expression for the reaction. For a reaction of order n, the rate law is typically expressed as: rate = k[A]^n, where [A] is the concentration of the reactant.
Rearrange the rate law expression to solve for the rate constant, k. This can be done by dividing the rate by the concentration raised to the power of the reaction order: k = rate / [A]^n.
Substitute the given values from the figure into the rearranged rate law expression. Ensure that the units are consistent with the order of the reaction.
Calculate the value of k, ensuring that the final answer is expressed with two significant figures, as required by the problem.
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