Consider the system SO3(g) ⇌SO2(g)+(1)/(2) O2(g) ΔH=98.9 kJ (a) Predict whether the forward o

step 1 Okay, so in this first step, we're going to add a product. Since that means that we have too muc

Consider the system SO3(g) ⇌SO2(g)+(1)/(2) O2(g) ΔH=98.9...

Consider the system $$ \mathrm{SO}_{3}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \quad \Delta H=98.9 \mathrm{~kJ} $$ (a) Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by (1) adding oxygen gas. (2) compressing the system at constant temperature. (3) adding argon gas. (4) removing $\mathrm{SO}_{2}(g)$. (5) decreasing the temperature. (b) Which of the above factors will increase the value of $K$ ? Which will decrease it?

Consider the system
$$
\mathrm{SO}_{3}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \quad \Delta H=98.9 \mathrm{~kJ}
$$
(a) Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by
(1) adding oxygen gas.
(2) compressing the system at constant temperature.
(3) adding argon gas.
(4) removing $\mathrm{SO}_{2}(g)$.
(5) decreasing the temperature.
(b) Which of the above factors will increase the value of $K$ ? Which will decrease it?

Key Concepts

Le Chatelier's Principle

This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium will shift to counteract the imposed change. It applies broadly to changes in concentration, pressure, volume, or temperature, allowing predictions about the direction in which the reaction will shift to re-establish equilibrium.

Equilibrium Constant and Temperature Dependence

The equilibrium constant (K) for a reaction depends solely on temperature. Changes in temperature alter the balance of the reaction’s forward and reverse rates, thereby changing K. For endothermic reactions, an increase in temperature increases K, while a decrease in temperature decreases K.

Pressure and Volume Effects in Gaseous Equilibria

In gas-phase reactions, changes in total pressure or volume affect the equilibrium position by altering the partial pressures of the reactants and products. According to Le Chatelier's Principle, a decrease in volume (or increase in pressure) will favor the direction that produces fewer moles of gas, while an increase in volume will favor the side with more moles.

Effects of Changing Concentrations

Altering the concentration of reactants or products disturbs the equilibrium. Adding a product or removing a reactant causes the equilibrium to shift toward the opposite side to restore balance. This concept is key in predicting how external changes affect the system’s overall reaction direction.

Role of Inert Gases in Equilibrium Systems

The addition of inert gases, such as argon, does not participate in the reaction and typically does not affect the equilibrium position if the volume remains constant. However, if added at constant pressure, inert gases can change the total volume and thereby indirectly affect the equilibrium of gas-phase reactions.

Transcript

Please give Ace some feedback