UndergradGuy7

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heat + CaSO3(s) <-> CaO(s) + SO2(g)

What change will cause an increase in the pressure of SO2(g) when equilibrium is re-established?

A. increase the reaction temperature
B. adding some more CaSO3
C. decreasing the volume of the container
D. removing some of the CaO(s)

I get how each would shift the reaction. A, C, and D would shift it to the right. B would shift it to the left.

Does this have nothing to do with shifting of the equilibrium? Do they just mean that higher temp = molecules move faster so higher pressure?
 
Last edited:
Jun 14, 2009
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heat + CaSO3(s) <-> CaO(s) + SO2(g)

What change will cause an increase in the pressure of SO2(g) when equilibrium is re-established?

A. increase the reaction temperature
B. adding some more CaSO3
C. decreasing the volume of the container
D. removing some of the CaO(s)

I get how each would shift the reaction. A, C, and D would shift it to the right. B would shift it to the left.

Does this have nothing to do with shifting of the equilibrium? Do they just mean that higher temp = molecules move faster so higher pressure?
I don't believe solids are considered to have any impact on the chemical equilibrium. Therefore B and D have no effect, C shifts to the left with no dynamic change in actual pressure, and A shifts to the right.
 

AmpedUp

The Legend Still Lives
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Dec 1, 2009
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Boyle's Gas Law will help you understand this kind of problem...

when pressure is increased, the volume is decreased (with respect to SO2)...