A catalyst speeds up a reaction by providing an alternative reaction pathway with a lower activation energy. While a catalyst accelerates both the forward and reverse reactions equally, it does not change the position of equilibrium. In other words, it helps the reaction reach equilibrium faster, but the equilibrium concentrations of reactants and products remain the same. Think of it like this: the catalyst is a shortcut; you still end up at the same destination (equilibrium), but you get there much quicker!
Match the term with its definition:
| Term | Definition |
|---|---|
| 1. Catalyst | A. The state where the rates of forward and reverse reactions are equal. |
| 2. Activation Energy | B. A substance that speeds up a reaction without being consumed. |
| 3. Equilibrium | C. The minimum energy required for a reaction to occur. |
| 4. Reaction Rate | D. A pathway with lower activation energy. |
| 5. Alternative Pathway | E. The speed at which reactants are converted to products. |
Match the letters and numbers to create the correct pairs.
Catalysts increase the __________ of a reaction by lowering the __________. They affect the __________ at which equilibrium is reached but do not change the __________ position.
Explain why a catalyst does not shift the equilibrium position. Use the concepts of forward and reverse reaction rates in your explanation.
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