Multiple Choice
How does a catalyst affect the activation energy of a chemical reaction?
36
views
15. Chemical Kinetics
Catalyst
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which statement about catalysts is NOT true?
A
Catalysts change the equilibrium position of a chemical reaction.
B
Catalysts lower the activation energy required for a reaction to occur.
C
Catalysts increase the rate of a chemical reaction without being consumed in the process.
D
Catalysts can be either homogeneous or heterogeneous.
Verified step by step guidance1
Understand the role of a catalyst in a chemical reaction: a catalyst provides an alternative reaction pathway with a lower activation energy, which increases the reaction rate.
Recall that catalysts do NOT change the equilibrium position of a reaction; they only help the system reach equilibrium faster by speeding up both the forward and reverse reactions equally.
Recognize that catalysts are not consumed during the reaction, meaning they remain unchanged after the reaction and can be used repeatedly.
Know the difference between homogeneous catalysts (in the same phase as reactants) and heterogeneous catalysts (in a different phase), both of which are valid types of catalysts.
Evaluate each statement based on these principles to identify the one that is NOT true: the statement claiming catalysts change the equilibrium position is incorrect.
1:59mWatch next
Master Catalyzed vs. Uncatalyzed Reactions with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
