Question

part 1 of 3
the following statements, i-iii, refer to the following reaction occurring in a rigid container:
2so₂(g) + o₂(g) ⇌ 2so₃(g) δh = -197.8 kj/mol
select if each statement is true or false.
i. increasing the temperature will cause the reaction to shift to the right in order to restore equilibrium.
true
false
part 2 of 3
ii. adding oxygen gas would cause the reaction to shift to the right in order for equilibrium to be restored.
true
false
part 3 of 3
iii. adding 2 l xe(g) would cause the reaction to shift to the right, i.e. towards the lesser number of moles of gas.
true
false

Explanation:

• For statement I:
• The reaction \(2SO_{2}(g)+O_{2}(g)

ightleftharpoons2SO_{3}(g)\) has \(\Delta H=- 197.8\ kJ/mol\), which means it is exothermic.

• According to Le - Chatelier's principle, increasing the temperature in an exothermic reaction will shift the equilibrium to the left (to absorb the added heat), not to the right.
• For statement II:
• Adding \(O_{2}\) (a reactant) increases the concentration of reactants.
• By Le - Chatelier's principle, the system will try to reduce this change, so the reaction will shift to the right (to consume the added \(O_{2}\)).
• For statement III:
• Adding \(Xe(g)\) (an inert gas) in a rigid container does not change the partial pressures of \(SO_{2}\), \(O_{2}\), or \(SO_{3}\).
• Since the reaction quotient \(Q = \frac{P_{SO_{3}}^{2}}{P_{SO_{2}}^{2}P_{O_{2}}}\) (where \(P\) represents partial pressure) is not affected, the equilibrium does not shift.

Answer:

• I. False
• II. True
• III. False