Chapter 58

A student says: "In the overall reaction given in Model 1 , two molecules react. Therefore, the rate law for the reaction should be: $$ \text { rate }=k_{\text {experimental }}\left(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CBr}\right)\left(\mathrm{OH}^{-}\right) $$ Explain why this student is not correct.

Note that the rate law given at the end of the Information section is second order in \(\mathrm{NO}\) and first order in \(\mathrm{O}_{2}\), as is the experimental rate law. What relationship must exist between \(k_{\exp }, k_{2}\) and \(K\) for the proposed mechanism to be consistent with the experimental rate law?

For a certain chemical reaction \(\Delta G^{\circ}=200 \mathrm{~kJ} / \mathrm{mol}\). When the reactants are mixed, no chemical reaction is apparent. Is this reaction under thermodynamic or kinetic control?

For a certain chemical reaction \(\Delta G^{\circ}=-200 \mathrm{~kJ} / \mathrm{mol}\). When the reactants are mixed, no chemical reaction is apparent. Is this reaction under thermodynamic or kinetic control?

What one feature of a reaction coordinate diagram is indicative of kinetic control of a reaction? Explain your reasoning. i) \(\quad \Delta H^{\circ}<0\) ii) \(\quad \Delta H^{\circ}>0\) iii) Activation energy is large iv) Activation energy is small