How do the following changes affect the value of the equilibrium constant for a gas-phase exothermic reaction: (a) removal of a reactant, (b) removal of a product?

Verified step by step guidance

1. Step 1: Understand the nature of the equilibrium constant (K). The equilibrium constant is a ratio of the concentrations of products to reactants, each raised to the power of their stoichiometric coefficients, at equilibrium. It is only affected by changes in temperature.
2. Step 2: Recognize that the equilibrium constant (K) is not affected by changes in concentration, pressure, or volume. These changes can shift the position of equilibrium but do not change the value of K.
3. Step 3: Consider the effect of removing a reactant. According to Le Chatelier's Principle, removing a reactant will shift the equilibrium position to the left (toward the reactants) to counteract the change, but the value of K remains unchanged.
4. Step 4: Consider the effect of removing a product. Similarly, removing a product will shift the equilibrium position to the right (toward the products) to counteract the change, but again, the value of K remains unchanged.
5. Step 5: Conclude that for both scenarios (a) removal of a reactant and (b) removal of a product, the equilibrium constant (K) remains unchanged because K is only affected by temperature changes, not by changes in concentration of reactants or products.