QuestionWhat happens to the equilibrium when $\mathrm{HI}$ gas is added to the system: A, B, C, or D? $51.8 \mathrm{~kJ}+\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})$

Studdy Solution

STEP 1

Assumptions1. The system is initially at equilibrium. . The system obeys Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
3. $\mathrm{HI}$ gas is added to the system.

STEP 2

According to Le Chatelier's principle, if a system at equilibrium is disturbed, the system will adjust itself to reduce the disturbance. In this case, the disturbance is the addition of $\mathrm{HI}$ gas.

STEP 3

Since $\mathrm{HI}$ gas is added to the system, the system will try to reduce the concentration of $\mathrm{HI}$ gas to reestablish equilibrium.

STEP 4

The reaction can reduce the concentration of $\mathrm{HI}$ gas by shifting to the left (reactants). This will consume $\mathrm{HI}$ gas and produce $\mathrm{H}_{2}$ and $\mathrm{}_{2}$ .

STEP 5

Therefore, the reaction shifts to the left (reactants) and the concentrations of $\mathrm{H}_{2}$ and $\mathrm{}_{2}$ increase.So, the correct answer is D. The reaction shifts to the left (reactants) and the concentrations of $\mathrm{H}_{2}$ and $\mathrm{}_{2}$ increase.

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QuestionWhat happens to the equilibrium when $\mathrm{HI}$ gas is added to the system: A, B, C, or D? $51.8 \mathrm{~kJ}+\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})$

Studdy Solution

STEP 1

Assumptions1. The system is initially at equilibrium. . The system obeys Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
3. $\mathrm{HI}$ gas is added to the system.

STEP 2

According to Le Chatelier's principle, if a system at equilibrium is disturbed, the system will adjust itself to reduce the disturbance. In this case, the disturbance is the addition of $\mathrm{HI}$ gas.

STEP 3

Since $\mathrm{HI}$ gas is added to the system, the system will try to reduce the concentration of $\mathrm{HI}$ gas to reestablish equilibrium.

STEP 4

The reaction can reduce the concentration of $\mathrm{HI}$ gas by shifting to the left (reactants). This will consume $\mathrm{HI}$ gas and produce $\mathrm{H}_{2}$ and $\mathrm{}_{2}$ .

STEP 5

Therefore, the reaction shifts to the left (reactants) and the concentrations of $\mathrm{H}_{2}$ and $\mathrm{}_{2}$ increase.So, the correct answer is D. The reaction shifts to the left (reactants) and the concentrations of $\mathrm{H}_{2}$ and $\mathrm{}_{2}$ increase.

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QuestionWhat happens to the equilibrium when HI\mathrm{HI}HI gas is added to the system: A, B, C, or D? 51.8 kJ+H2( g)+I2( g)⇌2HI(g)51.8 \mathrm{~kJ}+\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})51.8 kJ+H2​( g)+I2​( g)⇌2HI(g)

Studdy Solution

STEP 1

Assumptions1. The system is initially at equilibrium. . The system obeys Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.3. HI\mathrm{HI}HI gas is added to the system.

STEP 2

According to Le Chatelier's principle, if a system at equilibrium is disturbed, the system will adjust itself to reduce the disturbance. In this case, the disturbance is the addition of HI\mathrm{HI}HI gas.

STEP 3

Since HI\mathrm{HI}HI gas is added to the system, the system will try to reduce the concentration of HI\mathrm{HI}HI gas to reestablish equilibrium.

STEP 4

The reaction can reduce the concentration of HI\mathrm{HI}HI gas by shifting to the left (reactants). This will consume HI\mathrm{HI}HI gas and produce H2\mathrm{H}_{2}H2​ and 2\mathrm{}_{2}2​.

STEP 5

Therefore, the reaction shifts to the left (reactants) and the concentrations of H2\mathrm{H}_{2}H2​ and 2\mathrm{}_{2}2​ increase.So, the correct answer is D. The reaction shifts to the left (reactants) and the concentrations of H2\mathrm{H}_{2}H2​ and 2\mathrm{}_{2}2​ increase.

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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 $\mathrm{HI}$ gas is added to the system: A, B, C, or D? $51.8 \mathrm{~kJ}+\mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{HI}(\mathrm{g})$

Assumptions1. The system is initially at equilibrium. . The system obeys Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
3. $\mathrm{HI}$ gas is added to the system.

According to Le Chatelier's principle, if a system at equilibrium is disturbed, the system will adjust itself to reduce the disturbance. In this case, the disturbance is the addition of $\mathrm{HI}$ gas.

Since $\mathrm{HI}$ gas is added to the system, the system will try to reduce the concentration of $\mathrm{HI}$ gas to reestablish equilibrium.

The reaction can reduce the concentration of $\mathrm{HI}$ gas by shifting to the left (reactants). This will consume $\mathrm{HI}$ gas and produce $\mathrm{H}_{2}$ and $\mathrm{}_{2}$ .

Therefore, the reaction shifts to the left (reactants) and the concentrations of $\mathrm{H}_{2}$ and $\mathrm{}_{2}$ increase.So, the correct answer is D. The reaction shifts to the left (reactants) and the concentrations of $\mathrm{H}_{2}$ and $\mathrm{}_{2}$ increase.