Question

Reaction 3 represents the equilibrium between Co2t coordination complexes in mixtures of 2-propanol and methanol. Cotet + 3M = Cooct + P Reaction 3 1. For beakers A-E: a) Do you expect Key to be the same for each beaker? Explain. b) Did you find that Keg is indeed constant for these solutions? Briefly explain, stating your criteria for constancy c) How did increasing the proportion of methanol in the solutions affect the (Cotet]? Is this effect consistent with Le Chatelier's principle? Briefly explain. 2. For beakers C and F (the two solutions with the same composition): a) Do you expect Key to be the same for beakers C and F? Explain. b) How did increasing the temperature affect the [Cotet]? c) How did increasing the temperature affect Keg? d) Determine the sign of AHan for the conversion of Coret to Cooct (Reaction 3). Briefly explain.

Please answer question 1 & 2 based on the data provided

Answer 1

1) Ans :

a) As the equilibrium constant,K​​​​eq depend only on the temperature of the system,we can expect same value of Keq  from beaker A to E as they have the same temperature(temperature of E is almost same with the other four).

b) Yes. The value of K​​​​​​eq​ will be constant for all the solution from beaker A to E as they have the same temperature.

c) If methanol is added to the equilibrium mixture, the equilibrium position will shift to the right. This will increase the relative proportion of Co​​​​oct and shift the equilibrium to the octahedral side.

Yes. Because as the concentration of methanol changes, the other chemicals also shift to counteract that changes (Le Chatelier's principle, '' a change made to a chemical system at equilibrium will cause the equilibrium position to shift in a way that will reduce the effect of the change ").

2)Ans :

a) No. The value of K​​​​​​​​​​eq  will be different for beaker C and F because both the beakers have different temperatures.(beaker C-26°C, beaker F- 4°C)

b) The increase in temperature will effect the molecule to move more freely and collide with each other and thus increases the concentration. So, [Co​tet ​​​​​​] increases with increasing temperature.

c) We have a relation, K​​​​​​eq  = exp( -∆G/ RT )

where ∆G is change in the Gibbs free energy and R is the gas constant.

By this relation, we can say that K​​​​​​eq is inversely proportional to the temperature. An increase in temp. will decrease K​​​​​​eq value and vice-versa.

d) I need more information to answer this question.