Question

1. Explain in terms of rate laws and/or reaction quotients why the product’s
low solubility favors the forward reaction over the reverse. The forward rate law
is rate = k[maleic acid]n and the reverse rate law is: rate = k[fumaric acid]n.
Consider how the rate laws are affected by the respective solubilities.

2. Decolorizing carbon, a solid which was used in the recrystallization experiment, works by bonding with polar compounds. Predict the consequences if it is used to purify the crystallized fumaric acid product (polar).

I need help with these two question, thank you.