Relationship Between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G

For the reaction \[\ce{A(g) <=> 2B(g)}\] the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500, at 1000 K.

[Given: R = 0.0831 L atm mol⁻¹ K⁻¹]

K_p for the reaction at 1000 K is:

For the reaction \[\ce{2A <=> B + C}\], K_c = 4 × 10⁻³. At a given time, the composition of reaction mixture is:

[A] = [B] = [C] = 2 × 10⁻³ M

Then, which of the following is correct?

Write a relation between ∆G and Q and define the meaning term and answer the following:

Explain the effect of increase in pressure in terms of reaction quotient Q. for the reaction: \[\ce{CO (g) + 3H2 (g) ⇌ CH4 (g) + H2O (g)}\]

Write a relation between ∆G and Q and define the meaning term and answer the following:

Why a reaction proceeds forward when Q < K and no net reaction occurs when Q = K.