- Joined
- Jun 22, 2009
- Messages
- 397
- Reaction score
- 180
Which of the following will increase the value of the equilibrium constant for the following reaction?
CaCO3(s) <-> CaO(s) + CO2(g) Change in H=178 kJ
A) adding CaCO3
B) Removing CO2
C) Increasing Temperature
D) Decreasing temperature
Is my logic accurate here: The only thing that can change the equilibrium constant is temperature
So that eliminates A and B
Now we make the Keq equation.
Keq=[CO2] because it is the only gaseous or aqueous substance present.
We then see that change in H is positive. So it is an endothermic rxn and heat can be a reactant. Therefore if you increase temperature, the equation will shift to the right increasing amount of CO2, changing the Keq.
Is this right? Just looking for some insight. Thanks a lot.
CaCO3(s) <-> CaO(s) + CO2(g) Change in H=178 kJ
A) adding CaCO3
B) Removing CO2
C) Increasing Temperature
D) Decreasing temperature
Is my logic accurate here: The only thing that can change the equilibrium constant is temperature
So that eliminates A and B
Now we make the Keq equation.
Keq=[CO2] because it is the only gaseous or aqueous substance present.
We then see that change in H is positive. So it is an endothermic rxn and heat can be a reactant. Therefore if you increase temperature, the equation will shift to the right increasing amount of CO2, changing the Keq.
Is this right? Just looking for some insight. Thanks a lot.