Catalysts alter reaction rates without changing equilibrium position

Steps:

• Identify the reaction as gaseous reactants producing one gas and one liquid product, so rate likely measured by R(g) volume or pressure.
• Assume diagram shows faster R production in experiment 2, indicating higher rate.
• Evaluate options: pressure affects rate via collisions; catalyst changes activation energy; removing S shifts equilibrium by Le Chatelier's principle.
• Select option matching rate change without stoichiometry alteration.

Why B is correct:

• Catalysts lower activation energy, increasing rate constant (k) per Arrhenius equation, explaining faster R formation in experiment 2.

Why the others are wrong:

• A: Lower pressure decreases collision frequency, slowing rate, opposite of faster production.
• C: Removing S shifts equilibrium right, increasing R yield but not necessarily rate.
• D: Insufficient information provided.

Final answer: B