Chemical equilibrium combined

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Hydrogen gas and iodine gas are introduced into a flask, which is then sealed and allowed to reach dynamic chemical equilibrium.
The balanced equation is:

H2(g) + I2(g) ⇌ 2HI(g).

Which one of the graphs shows how the rates of the forward and reverse reactions change with time?

Which of the following is true regarding the concentration of products, for a chemical system at equilibrium?

The concentrations of products will not change because there are no more reactants.

The concentrations of products will not change because the limiting reagent is gone.

The concentrations of products will not change because the forward and reverse rates are equal.

The concentrations of products will change continually because of reversibility.

For the following system at equilibrium, which statement is INCORRECT?

Only one reaction will be affected by a change in temperature

It is a homogeneous equilibrium

The forward reaction is exothermic

The total change in enthalpy for the products is -184 kJ

Consider the amount (mol) vs. time graph for the closed system containing the gases of equation A at room temperature. The volume of the container is 1 dm3.
At which of the following time(s) is the the system NOT in equilibrium?

A disturbance to temperature was made at 10 minutes. Which reaction was favoured?

reverse reaction

forward reaction

Therefore, considering your answer above, what temperature change was made at 10 minutes?

Temperature was increased

Temperature was decreased

Given the following system at equilibrium:

The addition of Cl- ions will cause the concentration of Ag+(aq) to

Decrease as the amount of AgCl(s) increases

Increase as the amount of AgCl(s) increases

Decrease as the amount of AgCl(s) decreases

Increase as the amount of AgCl(s) decreases

Given the following system at equilibrium:

Increasing the concentration of N2(g) will increase the forward reaction rate due to:

An increase in the number of effective collisions

A decrease in the number of effective collisions

A decrease in the activation energy

An increase in the activation energy

Consider this system at equilibrium:

What colour could the gas mixture possibly be at equilibrium?

No colour change occurs

The solution turns more pink

The solution turns more blue

The solution turns colourless

What disturbance was made at 8 minutes?

SO2 was added into the system

SO2 was removed from the system

SO3 was removed from the system

SO3 was added into the system

What disturbance was made at 15 minutes?

Temperature was decreased

Temperature was increased

SO3 was removed from the system

SO3 was added into the system

Which reaction was favoured at 15 minutes?

Reverse reaction

Forward reaction

Increasing the pressure in a gaseous system at equilibrium causes .....

The reverse reaction rate to increase

All of these options are correct

The forward reaction rate to increase

The concentration of the gases to increase

Consider the Haber reaction system at equilibrium.

What happens when pressure is decreased?

The yield of ammonia increases

The reverse reaction is favoured.

Nitrogen gets used up more quickly

The reverse reaction speeds up

Consider the following system in equilibrium.

Pressure is increased by reducing the volume of the container.
What does NOT happen as a result?

All of these things happen as a result

The forward reaction is favoured

All the gases increase in concentration

Both reaction rates increase

Consider the following graph.
What is NOT a possible cause of the disturbance?

Increase in concentration of reactants

Increase in pressure

Increase in temperature

Decrease in volume

Consider the following system at equilibrium which experienced a disturbance.

What was the disturbance?

An increase in temperature

An increase in pressure of the system

A increase in concentration of the system

An increase in the volume of the system

What is the equilibrium constant Kc expression for the following balanced equation?

Hydrogen gas and iodine gas are introduced into a flask, which is then sealed and allowed to reach dynamic chemical equilibrium. 
The balanced equation is: 

H2(g) + I2(g) ⇌ 2HI(g). 

Which one of the graphs shows how the rates of the forward and reverse reactions change with time?

Which of the following is true regarding the concentration of products, for a chemical system at equilibrium?

The concentrations of products will not change because there are no more reactants.

The concentrations of products will not change because the limiting reagent is gone.

The concentrations of products will not change because the forward and reverse rates are equal.

The concentrations of products will change continually because of reversibility.

For the following system at equilibrium, which statement is INCORRECT?
 

Only one reaction will be affected by a change in temperature

It is a homogeneous equilibrium

The forward reaction is exothermic

The total change in enthalpy for the products is -184 kJ

Consider the amount (mol) vs. time graph for the closed system containing the gases of equation A at room temperature. The volume of the container is 1 dm3.
At which of the following time(s) is the the system NOT in equilibrium?

7 min

15 min

12 min

3 min

18 min

A disturbance to temperature was made at 10 minutes. Which reaction was favoured?

reverse reaction

forward reaction

Therefore, considering your answer above, what temperature change was made at 10 minutes? 

Temperature was increased

Temperature was decreased

Given the following system at equilibrium:

The addition of Cl- ions will cause the concentration of Ag+(aq) to

Decrease as the amount of AgCl(s) increases

Increase as the amount of AgCl(s) increases

Decrease as the amount of AgCl(s) decreases

Increase as the amount of AgCl(s) decreases

Given the following system at equilibrium:

Increasing the concentration of N2(g) will increase the forward reaction rate due to:

An increase in the number of effective collisions

A decrease in the number of effective collisions

A decrease in the activation energy

An increase in the activation energy

Consider this system at equilibrium:

What colour could the gas mixture possibly be at equilibrium?

none of these 

pale green

greenish yellow

all of these are possible

yellow

No colour change occurs

The solution turns more pink

The solution turns more blue

The solution turns colourless

What disturbance was made at 8 minutes?

SO2 was added into the system

SO2 was removed from the system

SO3 was removed from the system

SO3 was added into the system

What disturbance was made at 15 minutes?

Temperature was decreased

Temperature was increased

SO3 was removed from the system

SO3 was added into the system

Which reaction was favoured at 15 minutes?

Reverse reaction

Forward reaction

Increasing the pressure in a gaseous system at equilibrium causes .....

The reverse reaction rate to increase

All of these options are correct

The forward reaction rate to increase

The concentration of the gases to increase

Consider the Haber reaction system at equilibrium.  

What happens when pressure is decreased?

The yield of ammonia increases

The reverse reaction is favoured.

Nitrogen gets used up more quickly

The reverse reaction speeds up

Consider the following system in equilibrium.  


Pressure is increased by reducing the volume of the container. 
What does NOT happen as a result?

All of these things happen as a result

The forward reaction is favoured

All the gases increase in concentration

Both reaction rates increase

Consider the following graph.  
What is NOT a possible cause of the disturbance? 

Increase in concentration of reactants

Increase in pressure

Increase in temperature

Decrease in volume

Consider the following system at equilibrium which experienced a disturbance. 

What was the disturbance?

An increase in temperature

An increase in pressure of the system

A increase in concentration of the system

An increase in the volume of the system

What is the equilibrium constant Kc expression for the following balanced equation?

Chemical equilibrium combined

Chemical equilibrium combined

Hydrogen gas and iodine gas are introduced into a flask, which is then sealed and allowed to reach dynamic chemical equilibrium. The balanced equation is: H2(g) + I2(g) ⇌ 2HI(g). Which one of the graphs shows how the rates of the forward and reverse reactions change with time?

Which of the following is true regarding the concentration of products, for a chemical system at equilibrium?

For the following system at equilibrium, which statement is INCORRECT?

Consider the amount (mol) vs. time graph for the closed system containing the gases of equation A at room temperature. The volume of the container is 1 dm3.At which of the following time(s) is the the system NOT in equilibrium?

A disturbance to temperature was made at 10 minutes. Which reaction was favoured?

Therefore, considering your answer above, what temperature change was made at 10 minutes?

Given the following system at equilibrium:The addition of Cl- ions will cause the concentration of Ag+(aq) to

Given the following system at equilibrium:Increasing the concentration of N2(g) will increase the forward reaction rate due to:

Consider this system at equilibrium:What colour could the gas mixture possibly be at equilibrium?

What disturbance was made at 8 minutes?

What disturbance was made at 15 minutes?

Which reaction was favoured at 15 minutes?

Increasing the pressure in a gaseous system at equilibrium causes .....

Consider the Haber reaction system at equilibrium. What happens when pressure is decreased?

Consider the following system in equilibrium. Pressure is increased by reducing the volume of the container. What does NOT happen as a result?

Consider the following graph. What is NOT a possible cause of the disturbance?

Consider the following system at equilibrium which experienced a disturbance. What was the disturbance?

What is the equilibrium constant Kc expression for the following balanced equation?

Hydrogen gas and iodine gas are introduced into a flask, which is then sealed and allowed to reach dynamic chemical equilibrium.
The balanced equation is:

H2(g) + I2(g) ⇌ 2HI(g).

Which one of the graphs shows how the rates of the forward and reverse reactions change with time?

Consider the amount (mol) vs. time graph for the closed system containing the gases of equation A at room temperature. The volume of the container is 1 dm3.
At which of the following time(s) is the the system NOT in equilibrium?

Given the following system at equilibrium:

The addition of Cl- ions will cause the concentration of Ag+(aq) to

Given the following system at equilibrium:

Increasing the concentration of N2(g) will increase the forward reaction rate due to:

Consider this system at equilibrium:

What colour could the gas mixture possibly be at equilibrium?

Consider the Haber reaction system at equilibrium.

What happens when pressure is decreased?

Consider the following system in equilibrium.

Pressure is increased by reducing the volume of the container.
What does NOT happen as a result?

Consider the following graph.
What is NOT a possible cause of the disturbance?

Consider the following system at equilibrium which experienced a disturbance.

What was the disturbance?