QuestionWhat happens to the equilibrium when $\mathrm{H}_{2}$ gas is added to this reaction: $51.8 \mathrm{~kJ}+\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}$ ?

Studdy Solution

STEP 1

Assumptions1. The system is initially at equilibrium. . $\mathrm{H}_{}$ gas is added to the system.
3. The system adjusts to reestablish equilibrium according to Le Chatelier's principle.

STEP 2

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In this case, we have added extra $\mathrm{H}_{2}$ gas to the system.

STEP 3

According to Le Chatelier's principle, the system will try to decrease the concentration of $\mathrm{H}_{2}$ gas to reestablish equilibrium. This can be achieved by shifting the equilibrium to the right, towards the products, where $\mathrm{H}_{2}$ is consumed.

STEP 4

When the equilibrium shifts to the right, the concentration of $\mathrm{HI}$ , the product, will increase.

STEP 5

Therefore, the system adjusts to reestablish equilibrium by shifting the reaction to the right (products) and the concentration of $\mathrm{HI}$ increases.
The correct answer is B. The reaction shifts to the right (products) and the concentration of $\mathrm{HI}$ increases.

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QuestionWhat happens to the equilibrium when $\mathrm{H}_{2}$ gas is added to this reaction: $51.8 \mathrm{~kJ}+\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}$ ?

Studdy Solution

STEP 1

Assumptions1. The system is initially at equilibrium. . $\mathrm{H}_{}$ gas is added to the system.
3. The system adjusts to reestablish equilibrium according to Le Chatelier's principle.

STEP 2

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In this case, we have added extra $\mathrm{H}_{2}$ gas to the system.

STEP 3

According to Le Chatelier's principle, the system will try to decrease the concentration of $\mathrm{H}_{2}$ gas to reestablish equilibrium. This can be achieved by shifting the equilibrium to the right, towards the products, where $\mathrm{H}_{2}$ is consumed.

STEP 4

When the equilibrium shifts to the right, the concentration of $\mathrm{HI}$ , the product, will increase.

STEP 5

Therefore, the system adjusts to reestablish equilibrium by shifting the reaction to the right (products) and the concentration of $\mathrm{HI}$ increases.
The correct answer is B. The reaction shifts to the right (products) and the concentration of $\mathrm{HI}$ increases.

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QuestionWhat happens to the equilibrium when H2\mathrm{H}_{2}H2​ gas is added to this reaction: 51.8 kJ+H2+I2⇌2HI51.8 \mathrm{~kJ}+\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}51.8 kJ+H2​+I2​⇌2HI?

Studdy Solution

STEP 1

Assumptions1. The system is initially at equilibrium. . H\mathrm{H}_{}H​ gas is added to the system.3. The system adjusts to reestablish equilibrium according to Le Chatelier's principle.

STEP 2

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In this case, we have added extra H2\mathrm{H}_{2}H2​ gas to the system.

STEP 3

According to Le Chatelier's principle, the system will try to decrease the concentration of H2\mathrm{H}_{2}H2​ gas to reestablish equilibrium. This can be achieved by shifting the equilibrium to the right, towards the products, where H2\mathrm{H}_{2}H2​ is consumed.

STEP 4

When the equilibrium shifts to the right, the concentration of HI\mathrm{HI}HI, the product, will increase.

STEP 5

Therefore, the system adjusts to reestablish equilibrium by shifting the reaction to the right (products) and the concentration of HI\mathrm{HI}HI increases.The correct answer is B. The reaction shifts to the right (products) and the concentration of HI\mathrm{HI}HI increases.

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Studdy solves anything!

Start learning now

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

QuestionWhat happens to the equilibrium when $\mathrm{H}_{2}$ gas is added to this reaction: $51.8 \mathrm{~kJ}+\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}$ ?

Assumptions1. The system is initially at equilibrium. . $\mathrm{H}_{}$ gas is added to the system.
3. The system adjusts to reestablish equilibrium according to Le Chatelier's principle.

Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In this case, we have added extra $\mathrm{H}_{2}$ gas to the system.

According to Le Chatelier's principle, the system will try to decrease the concentration of $\mathrm{H}_{2}$ gas to reestablish equilibrium. This can be achieved by shifting the equilibrium to the right, towards the products, where $\mathrm{H}_{2}$ is consumed.

When the equilibrium shifts to the right, the concentration of $\mathrm{HI}$ , the product, will increase.

Therefore, the system adjusts to reestablish equilibrium by shifting the reaction to the right (products) and the concentration of $\mathrm{HI}$ increases.
The correct answer is B. The reaction shifts to the right (products) and the concentration of $\mathrm{HI}$ increases.