Consider the following exothermic reaction at a state of equilibrium: C(s) + O 2

Question

Consider the following exothermic reaction at a state of equilibrium: C(s) + O2(g) <----> CO2(g) . Which of the following changes will cause value of the equilibrium constant Kc to change?

Increasing the container volume

Increasing the temperature

Removing O2

Adding solid carbon

All of these

2.

Which of the following should be the most soluble in benzene, C6H6?

CH3OH

H2O2

CCl4

HF

CH3NH2

Increasing the container volume

Increasing the temperature

Removing O2

Adding solid carbon

All of these

2.

Which of the following should be the most soluble in benzene, C6H6?

CH3OH

H2O2

CCl4

HF

CH3NH2

Explanation / Answer

Increasing the temperature is cause value of the equilibrium constant Kc to change.

2) the most soluble in benzene, is CCl4 because both are non-polar.

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