Answer: A catalyst lowers the activation energy of both forward and reverse reactions equally, so both rates increase proportionally and equilibrium is reached faster but at the same position.
- A A catalyst is said to selectively affect mainly the reverse reaction pathway, leaving the forward reaction rate largely untouched and unchanged under most conditions encountered
- B A catalyst lowers the activation energy of both forward and reverse reactions equally, so both rates increase proportionally and equilibrium is reached faster but at the same position
- C A catalyst is said to directly alter the fundamental numerical value of the reaction's equilibrium constant itself as frequently observed in practice in many documented cases according to conventional understanding
- D A catalyst is said to function effectively mainly on exothermic reactions and to have no useful effect on endothermic ones in routine practice overall in most cases under typical conditions
Correct answer: B. A catalyst lowers the activation energy of both forward and reverse reactions equally, so both rates increase proportionally and equilibrium is reached faster but at the same position
Explanation: Since a catalyst lowers the activation energy barrier equally for forward and reverse reactions, both rates speed up by the same factor, so equilibrium is reached sooner without shifting its position or changing K.
A typical adsorption isotherm: x/m (mass adsorbed per gram of adsorbent) rises steeply at low pressure, then flattens into a saturation plateau as the adsorbent surface fills up.
Concept context
Explore the chemistry that happens at interfaces, from catalysts that speed up industrial reactions to colloids like milk, smoke, and gels that surround us every day.