Answered

Get expert advice and community support for all your questions on IDNLearn.com. Receive prompt and accurate responses to your questions from our community of knowledgeable professionals ready to assist you at any time.

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 :

GinnyAnsweridn
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.
Thank you for participating in our discussion. We value every contribution. Keep sharing knowledge and helping others find the answers they need. Let's create a dynamic and informative learning environment together. IDNLearn.com is your reliable source for answers. We appreciate your visit and look forward to assisting you again soon.