Questions: Question 14 (1 point) When the concentrations of reactant molecules are increased, the rate of reaction increases. The best explanation for this phenomenon is that as the reactant concentration increases, the average kinetic energy of molecules increases. the frequency of molecular collisions increases. the rate constant increases. the activation energy increases. the order of reaction increases. Question 15 (1 point) 18 The following mechanism has been suggested for the reaction: H2O2 + 2 H+ + 2 I- → I2 + 2 H2O H2O2 + I- → HOI + OH- OH- + H+ → H2O HOI + H+ + I- → I2 + H2O Slow Fast Fast Identify all intermediates included in this mechanism. H+ and I- H+ and HOI HOI and OH- H+ only H2O and OH-

Transcript text: Question 14 (1 point) When the concentrations of reactant molecules are increased, the rate of reaction increases. The best explanation for this phenomenon is that as the reactant concentration increases, the average kinetic energy of molecules increases. the frequency of molecular collisions increases. the rate constant increases. the activation energy increases. the order of reaction increases. Question 15 (1 point) 18 The following mechanism has been suggested for the reaction: \[ \begin{array}{l} \mathrm{H}_{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{I}^{-} \rightarrow \mathrm{I}_{2}+2 \mathrm{H}_{2} \mathrm{O} \\ \mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{I}^{-} \rightarrow \mathrm{HOI}+\mathrm{OH}^{-} \\ \mathrm{OH}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{H}_{2} \mathrm{O} \\ \mathrm{HOI}+\mathrm{H}^{+}+\mathrm{I}^{-} \rightarrow \mathrm{I}_{2}+\mathrm{H}_{2} \mathrm{O} \end{array} \] Slow Fast Fast Identify all intermediates included in this mechanism. $\mathrm{H}^{+}$and $\mathrm{I}^{-}$ $\mathrm{H}^{+}$and HOI HOI and $\mathrm{OH}^{-}$ $\mathrm{H}^{+}$only $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{OH}^{-}$