Question

question 4
how can we figure out if a reaction is going to go forward or backward?
multiply q and k
compare the values of q and k
compare k to gibbs free energy
determine if q is greater than or less than 1
question 5
what happens to a reaction if qc < kc?
the reaction proceeds to the left, forming more reactants.
the reaction proceeds to the right, forming more products.
no change, the reaction is at equilibrium.
the reaction stops as it has reached its final state.

Explanation:

For Question 4:

• The reaction quotient \(Q\) and equilibrium constant \(K\) are compared. If \(Q K\), reaction goes backward; if \(Q=K\), reaction is at equilibrium. Multiplying \(Q\) and \(K\) is not relevant. Comparing \(K\) to Gibbs free energy (\(\Delta G=-RT\ln K\)) is for spontaneity (not direction in this context). \(Q\) compared to 1 is not the standard way to determine reaction direction.

For Question 5:

• When \(Q_c K_c\), reaction shifts left. If \(Q_c=K_c\), reaction is at equilibrium.

Answer:

Question 4: compare the values of Q and K
Question 5: The reaction proceeds to the right, forming more products.