Answered

Welcome to Westonci.ca, where your questions are met with accurate answers from a community of experts and enthusiasts. Our platform provides a seamless experience for finding reliable answers from a network of experienced professionals. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform.

Given the reaction:
[tex]\[ H_2O_2(l) \rightleftharpoons H_2(g) + O_2(g) \][/tex]
The forward reaction is endothermic.

Determine which of the following changes would result in equilibrium shifting towards the reactants:

I. Increase [tex]\( H_2 \)[/tex]
II. Decrease [tex]\( O_2 \)[/tex]
III. Add a catalyst
IV. Decrease the temperature
V. Increase [tex]\( H_2O_2 \)[/tex]

A. I and IV
B. I and II
C. II, III, and V
D. All

Sagot :

GinnyAnswer
To determine how the equilibrium will shift for the given reaction [tex]\( H_2O_2(l) \rightleftharpoons H_2(g) + O_2(g) \)[/tex], we need to apply Le Chatelier's Principle, which states that the equilibrium will shift in the direction that counteracts any imposed change.

1. Increase [tex]\( H_2 \)[/tex]:
- Increasing [tex]\( H_2 \)[/tex] will cause the equilibrium to shift towards the reactants to counteract the increase in [tex]\( H_2 \)[/tex] concentration by producing less [tex]\( H_2 \)[/tex] and [tex]\( O_2 \)[/tex], and more [tex]\( H_2O_2 \)[/tex].

2. Decrease [tex]\( O_2 \)[/tex]:
- Decreasing [tex]\( O_2 \)[/tex] should cause the equilibrium to shift towards the products to counteract the decrease by forming more [tex]\( H_2 \)[/tex] and [tex]\( O_2 \)[/tex], and using up more [tex]\( H_2O_2 \)[/tex].

3. Add a catalyst:
- Adding a catalyst does not shift the equilibrium position; it only speeds up the rate at which equilibrium is achieved for both forward and reverse reactions.

4. Decrease the temperature:
- Since the forward reaction is endothermic (absorbs heat), decreasing the temperature will shift the equilibrium towards the exothermic direction, which is the reverse reaction, forming more [tex]\( H_2O_2 \)[/tex].

5. Increase [tex]\( H_2O_2 \)[/tex]:
- Increasing [tex]\( H_2O_2 \)[/tex] will shift the equilibrium towards the products to counteract the increase in [tex]\( H_2O_2 \)[/tex] concentration by producing more [tex]\( H_2 \)[/tex] and [tex]\( O_2 \)[/tex].

Given these considerations, the changes resulting in the equilibrium shifting towards the reactants are:
I. Increase [tex]\( H_2 \)[/tex]
IV. Decrease the temperature

Thus, the correct answer is A. I and IV.
Visit us again for up-to-date and reliable answers. We're always ready to assist you with your informational needs. Thank you for visiting. Our goal is to provide the most accurate answers for all your informational needs. Come back soon. Westonci.ca is committed to providing accurate answers. Come back soon for more trustworthy information.