Solution Found!
The rate law for the reactionNO2( g) + CO( g) ? NO(g) +
Chapter 16, Problem 71P(choose chapter or problem)
The rate law for the reaction
is \(\text { rate }=k\left[\mathrm{NO}_{2}\right]^{2}\); one possible mechanism is shown on p. 537.
(a) Draw a reaction energy diagram for that mechanism, given that \(\Delta H_{\text {overall }}^{\circ}=226 \mathrm{~kJ} / \mathrm{mol}\).
(b) The following alternative mechanism has been proposed:
Is the alternative mechanism consistent with the rate law? Is one mechanism more reasonable physically? Explain.
Equation Transcription:
rate = 𝑘[NO2]2
= 226 kJ/mol
Text Transcription:
rate = 𝑘[NO_2]^2
Delta H_overall°= 226 kJ/mol
Questions & Answers
QUESTION:
The rate law for the reaction
is \(\text { rate }=k\left[\mathrm{NO}_{2}\right]^{2}\); one possible mechanism is shown on p. 537.
(a) Draw a reaction energy diagram for that mechanism, given that \(\Delta H_{\text {overall }}^{\circ}=226 \mathrm{~kJ} / \mathrm{mol}\).
(b) The following alternative mechanism has been proposed:
Is the alternative mechanism consistent with the rate law? Is one mechanism more reasonable physically? Explain.
Equation Transcription:
rate = 𝑘[NO2]2
= 226 kJ/mol
Text Transcription:
rate = 𝑘[NO_2]^2
Delta H_overall°= 226 kJ/mol
ANSWER:
Solution 71P
The rate law for the reaction
NO2( g) + CO( g) → NO(g) + CO2( g) is rate = A[NO2]2
Step 1
(a)We have to draw a reaction energy diagram for the above reaction, given that
= -226 kJ/mol
In this question it has been given that, the is -ve for this reaction. Hence the energy of the product is greater than the energy of the reactant. Thus it is an exothermic reaction. The energy level diagram with reaction coordinate in the X-axis and energy in the Y-axis is given below,