Answered

Welcome to Westonci.ca, where finding answers to your questions is made simple by our community of experts. Our platform provides a seamless experience for finding precise answers from a network of experienced professionals. Discover detailed answers to your questions from a wide network of experts on our comprehensive Q&A 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.
Your visit means a lot to us. Don't hesitate to return for more reliable answers to any questions you may have. Thank you for your visit. We're committed to providing you with the best information available. Return anytime for more. Get the answers you need at Westonci.ca. Stay informed by returning for our latest expert advice.