QuestionHow can you increase the formation of $\mathrm{H}_{2}$ in the reaction: $\mathrm{CH}_{4} + 2 \mathrm{H}_{2} \mathrm{S} \rightleftharpoons 4 \mathrm{H}_{2} + \mathrm{CS}_{2}$ ? Options: A. remove $\mathrm{CH}_{4}$ , B. remove $\mathrm{H}_{2} \mathrm{S}$ , C. remove $\mathrm{CS}_{2}$ , D. add $\mathrm{H}_{2}$ .

Studdy Solution

STEP 1

Assumptions1. The reaction is at equilibrium. . The reaction follows Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

STEP 2

We need to encourage more product, H2, to form from the reaction. According to Le Chatelier's Principle, we can shift the equilibrium to the right (towards the products) by either adding more reactants or removing some products.

STEP 3

Now, let's evaluate each of the given optionsA. remove CHB. remove H2C. remove CS2. add H2

STEP 4

Option A Removing CH4. According to Le Chatelier's Principle, if we remove some CH4, the reaction will shift to the left to replace the CH4, which would decrease the amount of H2.

STEP 5

Option B Removing H2. According to Le Chatelier's Principle, if we remove some H2, the reaction will shift to the left to replace the H2, which would decrease the amount of H2.

STEP 6

Option C Removing CS2. According to Le Chatelier's Principle, if we remove some CS2, the reaction will shift to the right to replace the CS2, which would increase the amount of H2.

STEP 7

Option D Adding H2. According to Le Chatelier's Principle, if we add more H2, the reaction will shift to the left to consume the added H2, which would decrease the amount of H2.

STEP 8

Based on the analysis of each option, the method that would encourage more H2 to form from the reaction is to remove CS2.
The solution is C remove CS2.

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Studdy Solution

STEP 1

Assumptions1. The reaction is at equilibrium. . The reaction follows Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

STEP 2

We need to encourage more product, H2, to form from the reaction. According to Le Chatelier's Principle, we can shift the equilibrium to the right (towards the products) by either adding more reactants or removing some products.

STEP 3

Now, let's evaluate each of the given optionsA. remove CHB. remove H2C. remove CS2. add H2

STEP 4

Option A Removing CH4. According to Le Chatelier's Principle, if we remove some CH4, the reaction will shift to the left to replace the CH4, which would decrease the amount of H2.

STEP 5

Option B Removing H2. According to Le Chatelier's Principle, if we remove some H2, the reaction will shift to the left to replace the H2, which would decrease the amount of H2.

STEP 6

Option C Removing CS2. According to Le Chatelier's Principle, if we remove some CS2, the reaction will shift to the right to replace the CS2, which would increase the amount of H2.

STEP 7

Option D Adding H2. According to Le Chatelier's Principle, if we add more H2, the reaction will shift to the left to consume the added H2, which would decrease the amount of H2.

STEP 8

Based on the analysis of each option, the method that would encourage more H2 to form from the reaction is to remove CS2.
The solution is C remove CS2.

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Studdy Solution

STEP 1

Assumptions1. The reaction is at equilibrium. . The reaction follows Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

STEP 2

We need to encourage more product, H2, to form from the reaction. According to Le Chatelier's Principle, we can shift the equilibrium to the right (towards the products) by either adding more reactants or removing some products.

STEP 3

Now, let's evaluate each of the given optionsA. remove CHB. remove H2C. remove CS2. add H2

STEP 4

Option A Removing CH4. According to Le Chatelier's Principle, if we remove some CH4, the reaction will shift to the left to replace the CH4, which would decrease the amount of H2.

STEP 5

Option B Removing H2. According to Le Chatelier's Principle, if we remove some H2, the reaction will shift to the left to replace the H2, which would decrease the amount of H2.

STEP 6

Option C Removing CS2. According to Le Chatelier's Principle, if we remove some CS2, the reaction will shift to the right to replace the CS2, which would increase the amount of H2.

STEP 7

Option D Adding H2. According to Le Chatelier's Principle, if we add more H2, the reaction will shift to the left to consume the added H2, which would decrease the amount of H2.

STEP 8

Based on the analysis of each option, the method that would encourage more H2 to form from the reaction is to remove CS2.The solution is C remove CS2.

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Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

Based on the analysis of each option, the method that would encourage more H2 to form from the reaction is to remove CS2.
The solution is C remove CS2.