How would you approach these questions 2. The following equilibrium system shows the reaction of sour gas with methane to produce carbon disulfide...

How would you approach these questions

2.

The following equilibrium system shows the reaction of sour gas with methane to produce carbon disulfide and hydrogen gas.

CH4(g)+2H2S(g)⇋CS2(g)+4H2(g)ΔrH=+232.5kJ

State what effect each of the following stresses will have on this system in terms of the amount of H2S(g) present at equilibrium.

stressamount of H2S(g)

Adding CH4(g)Choose...

increase

decrease

no change

Heating the system

Choose...

increase

decrease

no change

Adding H2(g)Choose...

increase

decrease

no change

Removing CS2(g)Choose...

increase

decrease

no change

Decreasing the pressure by increasing the volume of the containerChoose...

increase

decrease

no change

Cooling the systemChoose...

increase

decrease

no change

Decreasing the volume of the containerChoose...

increase

decrease

no change

Removing CH4(g))Choose...

increase

decrease

no change

3.

Use the following information to answer the next question.

A sealed container contains the following system at equilibrium.

2CO(g)+O2(g)⇋2CO2(g)+566kJ

For each of the following stresses, state the effect on the system. Does the stress favour the forward reaction, favour the reverse reaction, or have no effect on the position of equilibrium?

stressshift

Adding CO2(g)

Choose...

favours the forward reaction

favours the reverse reaction

no effect on the position of equilibrium

Heating the system

Choose...

favours the forward reaction

favours the reverse reaction

no effect on the position of equilibrium

Adding CO(g)

Choose...

favours the forward reaction

favours the reverse reaction

no effect on the position of equilibrium

Removing O2(g)

Choose...

favours the forward reaction

favours the reverse reaction

no effect on the position of equilibrium

Decreasing the pressure by increasing the volume of the container

Choose...

favours the forward reaction

favours the reverse reaction

no effect on the position of equilibrium

Cooling the system

Choose...

favours the forward reaction

favours the reverse reaction

no effect on the position of equilibrium

decreasing the volume of the container

Choose...

favours the forward reaction

favours the reverse reaction

no effect on the position of equilibrium

Removing CO2(g)

Choose...

favours the forward reaction

favours the reverse reaction

no effect on the position of equilibrium

4.

A sealed container contains the following system at equilibrium.

H2(g)+Br2(g)⇋2HBr(g)ΔrH=−36kJ

For each of the following stresses, state the effect on the system. Does the stress favour the forward reaction, favour the reverse reaction, or have no effect on the position of equilibrium?

stressshift

Adding Br2(g)

Choose...

favours the forward reaction

favours the reverse reaction 

no effect on the position of equilibrium

Heating the system

Choose...

favours the forward reaction

favours the reverse reaction 

no effect on the position of equilibrium

Adding HBr(g)

Choose...

favours the forward reaction

favours the reverse reaction 

no effect on the position of equilibrium

Removing H2(g)

Choose...

favours the forward reaction

favours the reverse reaction 

no effect on the position of equilibrium

Increasing the pressure by decreasing the volume of the container

Choose...

favours the forward reaction

favours the reverse reaction 

no effect on the position of equilibrium

Cooling the system

Choose...

favours the forward reaction

favours the reverse reaction 

no effect on the position of equilibrium

Increasing the volume of the container

Choose...

favours the forward reaction

favours the reverse reaction 

no effect on the position of equilibrium

Removing HBr(g)

Choose...

favours the forward reaction

favours the reverse reaction 

no effect on the position of equilibrium

5.

Sour gas, H2S(g), can establish the following equilibrium system under certain conditions:

2H2S(g)⇋2H2(g)+S2(g)

Disulfur, S2(g), is a violet coloured gas. Both sour gas and hydrogen gas are colourless.

State the effect each of the following stresses will have on this system in terms of the colour of the system: darker violet in colour, lighter violet in colour, or no change to the colour of the system.

stressshift

Adding H2(g)

Choose...

darker violet colour

lighter violet colour

no change to colour of system

Adding H2S(g)

Choose...

darker violet colour

lighter violet colour

no change to colour of system

Removing H2(g)

Choose...

darker violet colour

lighter violet colour

no change to colour of system

Increasing the pressure by decreasing the volume of the container

Choose...

darker violet colour

lighter violet colour

no change to colour of system

Increasing the volume of the container

Choose...

darker violet colour

lighter violet colour

no change to colour of system

Removing H2S(g)

Choose...

darker violet colour

lighter violet colour

no change to colour of system

Adding an inert gas

Choose...

darker violet colour

lighter violet colour

no change to colour of system

6.

The following equilibrium system was heated.

H2(g)+I2(g)+53kJ⇋2HI(g)

Identify the effect of the temperature increase on the concentration of HI and on the equilibrium constant (Kc) of this system.

Effect

Concentration of HI

Choose...

increases

decreases

Kc

Choose...

increases

decreases

9.The temperature of an endothermic reaction is decreased. Identify how this will affect the position of equilibrium and the the amount of products/reactants.

Effect

Position of equilibrium will

Choose...

shift left

shift right

no shift

The amount of products will

Choose...

increase

decrease

no change

The amount of reactants will

Choose...

increase

decrease

no change

10.

A quantity of hydrogen gas is added to this system at equilibrium.

3H2(g)+N2(g)⇋2NH3(g)

Identify the effect that the addition of hydrogen has on the concentration of NH3 and on the equilibrium constant (Kc) of this system.

Effect

Concentration of NH3

Choose...

increase

decrease

no change

Kc

Choose...

increase

decrease

no change

11.

Consider the following equilibrium:

4HCl(g)+2O2(g)⇋2Cl2(g)+4H2O(l)

HCl(g) is colourless and Cl2(g) is yellow. When the above equilibrium is heated, the yellow colour fades. From this it is logical to infer that the reaction is

Select one:

endothermic

exothermic

12.

Consider the following equilibrium:

BaS(s)⇋Ba2+(aq)+S2−(aq)

When Ba(NO3)2(aq) is added to this solution, the equilibrium shifts to the 

Choose...

left

right

 and the concentration of sulfide ions 

Choose...

increase

decrease

13.

When the volume of the container is increased the system will

Select one:

not shift

shift right

shift left

14.

Phosgene was a chemical weapon that caused approximately 85 000 deaths in World War I. It is still manufactured today and is used in the synthesis of polyurethanes. It is a tightly regulated substance. Phosgene is prepared by the reaction of carbon monoxide and chlorine and it establishes the following equilibrium:

CO(g)+Cl2(g)⇋COCl2(g)ΔrH=−9.93kJ

The following conditions would produce the highest yield of phosgene

Select one:

A)high temperature and high pressure

B)low temperature and low pressure

C)low temperature and high pressure

D)high temperature and low pressure

 .