Direction of Reaction to Reach Equilibrium

Some C6H5CH2OH is allowed to dissociate into C6H5CHO and H2 at 523 K. At equilibrium, [CH-CH2OH] = 0.206 M, and [CH3CHO] = [H2] = 5.18x10^-2 M. Additional CH3CH2OH is added so that [CH3CH,OH]new = 0.315 M and the system is allowed to once again reach equilibrium. C6H5CHOH(g) ⇌ C6H5CHO(g) + H2(g) K=1.30x10^-2 at 523 K. In which direction will the reaction proceed to reach equilibrium?

Final Answer:

The reaction will proceed from left to right to reach equilibrium.

Explanation:

Le Chatelier's principle states that a system at equilibrium will shift in a way that counteracts any changes imposed on it. In this case, additional CH3CH2OH is added to the system, increasing its concentration. According to the given equilibrium equation:

C6H5CHOH(g) ⇌ C6H5CHO(g) + H2(g)

The equilibrium constant (K) for this reaction is 1.30x10^-2 at 523 K. The concentrations at equilibrium are given as [CH3CH2OH] = 0.206 M, [CH3CHO] = [H2] = 5.18x10^-2 M.

When more CH3CH2OH is added, the concentration of CH3CH2OH increases to 0.315 M. To determine the direction of the shift, we compare the initial concentrations with the new concentrations:

[CH3CH2OH] initial = 0.206 M, [CH3CH2OH] new = 0.315 M

[CH3CHO] initial = [H2] initial = 5.18x10^-2 M, [CH3CHO] new = [H2] new = 5.18x10^-2 M

Since the concentration of CH3CH2OH has increased, the system will shift in the direction that consumes CH3CH2OH. This means that the reaction will proceed from left to right, converting more C6H5CH2OH into C6H5CHO and H2 until a new equilibrium is reached.

In which direction will the reaction proceed to reach equilibrium?

The reaction will proceed from left to right to reach equilibrium.