The rate of a reaction:

Question

BlackTom AI · Accepted Answer

To approach the question, I will evaluate what factors influence chemical reaction rates and then apply that to each option.
Option a: 'Is typically faster for reactions involving heavy isotopes.' In fact, reactions involving heavy isotopes often proceed more slowly due to the kinetic isotope effect, not faster. This makes the statement incorrect.
Option b: 'Is predicted by the magnitude of the Gibbs free energy.' The Gibbs free energy change tells us about spontaneity and thermodynamic favorability, not the rate of the reaction. Kinetics, including activation energy and collisions, governs rate, so this claim is inaccurate.
Option c: 'Is increased by increasing the reactive surface area.' This is true because a larger surface area provides more accessible sites for collisions and reactive encounters, thereby increasing the frequency of effective collisions and speeding up the reaction rate. This aligns with fundamental kinetics principles.
Option d: 'Is equal for both the forward and backward reaction in a disequilibrium state.' In a disequilibrium state, the system is not constrained to equal forward and reverse rates; only at equilibrium are the forward and backward rates equal. Therefore, stating equality in a disequilibrium state is incorrect.
Overall, the reasoning shows that option c correctly describes how surface area affects rate, while the other options conflict with established kinetic concepts.

The rate of a reaction:

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