Chapter 12: Problem 19
The central idea of the collision model is that molecules must collide in order to react. Give two reasons why not all collisions of reactant molecules result in product formation.
Chapter 12: Problem 19
The central idea of the collision model is that molecules must collide in order to react. Give two reasons why not all collisions of reactant molecules result in product formation.
All the tools & learning materials you need for study success - in one app.
Get started for freeUpon dissolving \(\operatorname{InCl}(s)\) in \(\mathrm{HCl}, \mathrm{In}^{+}(a q)\) undergoes a disproportionation reaction according to the following unbalanced equation: $$ \mathrm{In}^{+}(a q) \longrightarrow \operatorname{In}(s)+\mathrm{In}^{3+}(a q) $$ This disproportionation follows first-order kinetics with a halflife of \(667 \mathrm{~s}\). What is the concentration of \(\mathrm{In}^{+}(a q)\) after \(1.25 \mathrm{~h}\) if the initial solution of \(\mathrm{In}^{+}(a q)\) was prepared by dissolving \(2.38 \mathrm{~g} \operatorname{InCl}(s)\) in \(5.00 \times 10^{2} \mathrm{~mL}\) dilute HCl? What mass of \(\operatorname{In}(s)\) is formed after \(1.25 \mathrm{~h}\) ?
Consider a reaction of the type \(\mathrm{aA} \longrightarrow\) products, in which the rate law is found to be rate \(=k[\mathrm{~A}]^{3}\) (termolecular reactions are improbable but possible). If the first half-life of the reaction is found to be \(40 . \mathrm{s}\), what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a termolecular reaction: $$ \text { Rate }=\frac{-d[\mathrm{~A}]}{d t}=k[\mathrm{~A}]^{3} $$
Describe at least two experiments you could perform to determine a rate law.
Draw a rough sketch of the energy profile for each of the following cases: a. \(\Delta E=+10 \mathrm{~kJ} / \mathrm{mol}, E_{\mathrm{a}}=25 \mathrm{~kJ} / \mathrm{mol}\) b. \(\Delta E=-10 \mathrm{~kJ} / \mathrm{mol}, E_{\mathrm{a}}=50 \mathrm{~kJ} / \mathrm{mol}\) c. \(\Delta E=-50 \mathrm{~kJ} / \mathrm{mol}, E_{\mathrm{a}}=50 \mathrm{~kJ} / \mathrm{mol}\)
A certain first-order reaction is \(45.0 \%\) complete in \(65 \mathrm{~s}\). What are the values of the rate constant and the half-life for this process?
What do you think about this solution?
We value your feedback to improve our textbook solutions.