Asked by Aaron Guerra on Jul 25, 2024
Verified
In the reaction: N2 + 3 H2 ⇌ 2 NH3, the equilibrium constant is very small, yet ammonia (NH3) is readily produced. What conditions might be applied to make this happen?
A) A catalyst is added.
B) Product is removed as soon as it is formed.
C) All of the above.
D) None of the above.
Equilibrium Constant
A number that expresses the ratio of products to reactants at equilibrium for a chemical reaction, indicating the extent of the reaction.
Ammonia
A colorless gas with a characteristic pungent smell, consisting of nitrogen and hydrogen (NH3), used as a fertilizer and cleaning agent.
Catalyst
A material that accelerates the speed of a chemical reaction without experiencing any lasting chemical alteration.
- Recognize the roles of catalysts in chemical reactions and their effect on equilibrium without altering the position of equilibrium.
Verified Answer
JH
Jackson Hallman
Jul 29, 2024
Final Answer :
C
Explanation :
Adding a catalyst speeds up the reaction without affecting the equilibrium position, and removing the product as it forms shifts the equilibrium to the right, favoring the formation of more product. Both conditions can help in increasing the production of ammonia despite a small equilibrium constant.
Learning Objectives
- Recognize the roles of catalysts in chemical reactions and their effect on equilibrium without altering the position of equilibrium.