Question

match the statements with either graph a or b
a
reactants
products
potential energy
reaction progress
b
reactants
products
potential energy
reaction progress
the reaction that has a greater activation energy
the reaction that occurs faster
exothermic reaction
b a both a & b

Explanation:

Step1: Compare activation energies

The height of the energy - barrier from reactants to the transition state represents activation energy ($E_a$). In graph B, the $E_a$ value is larger as the peak is higher compared to graph A.

Step2: Analyze reaction speed

Reactions with lower activation energies occur faster. Since graph A has a lower $E_a$, the reaction in graph A occurs faster.

Step3: Determine exothermic reaction

In an exothermic reaction, the energy of the products is lower than the energy of the reactants ($\Delta H<0$). Both graph A and graph B show that the energy of the products is lower than that of the reactants, so both are exothermic reactions.

Answer:

The reaction that has a greater activation energy: B
The reaction that occurs faster: A
Exothermic reaction: Both A & B