難関大向け｜英語長文問題106（化学）144語＋和訳・解答解説

In everyday language, a catalyst “speeds things up,” but in chemistry its role is subtler and more consequential. A reaction proceeds only when molecules reach a high-energy transition state; the required activation energy acts like a toll that most collisions cannot pay. Catalysts provide an alternative pathway in which intermediates form and break apart in a controlled sequence, lowering that energetic barrier without changing the reaction’s final equilibrium. Because the catalyst is regenerated, tiny amounts can transform industrial economics: enzymes in fermentation, platinum in car exhaust converters, or metal complexes that stitch polymers from simple monomers. Yet catalysis is not magic. Selectivity matters as much as rate, since the fastest pathway may yield unwanted by-products. Modern research therefore designs catalytic surfaces and ligands that steer electrons, shape reactant orientation, and exploit solvent effects to favor one product over many, under practical temperatures and pressures.

Which TWO statements are NOT supported by the passage?

1. Catalysts lower activation barriers by offering a different reaction route.
2. They accelerate reactions yet do not shift the equilibrium position.
3. Even small catalyst amounts can have major industrial impact.
4. Catalysts are permanently consumed, so they must be constantly replaced.
5. Selectivity is crucial because faster routes may create unwanted products.
6. Current catalysis research ignores solvents and focuses only on temperature.