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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
.
