Equilibrium?
2SO2 (g) + O2>>>(g) 2SO3
(g) ∆Hο= –200 kJ
According to the above information, what temperature and pressure conditions produce the
greatest amount of SO3? Give explanation
Temperature Pressure
A. low low
B. low high
C. high high
D. high low
three gas volumes on left, two on right. High pressure makes go right
reaction gives off heat, lower temp makes it go right
To determine the temperature and pressure conditions that produce the greatest amount of SO3 in the given reaction, we need to understand the factors that affect the equilibrium position.
According to Le Chatelier's principle, the equilibrium position will shift in a direction that reduces the impact of any changes made to the system. In this reaction, the formation of SO3 is an exothermic reaction, meaning it releases heat. The negative value for ∆Hο indicates that the reaction is exothermic.
1. Temperature:
According to Le Chatelier's principle, increasing the temperature will favor the reaction that consumes heat. In this case, increasing the temperature will shift the equilibrium in the reverse direction, favoring the formation of reactants (SO2 and O2) rather than products (SO3). Therefore, a lower temperature will favor the formation of SO3.
2. Pressure:
In this reaction, the number of moles of gas is constant on both sides of the equation. So, changes in pressure will not affect the equilibrium position.
Based on the information above, the answer is option A: low temperature and low pressure conditions will produce the greatest amount of SO3.
To determine the temperature and pressure conditions that produce the greatest amount of SO3, we need to consider Le Chatelier's principle, which predicts how a system at equilibrium will respond to changes in temperature, pressure, or concentration.
In the given reaction: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) ΔHο=-200 kJ
According to Le Chatelier's principle, an increase in temperature will favor the endothermic reaction to absorb the excess heat, while a decrease in temperature will favor the exothermic reaction to generate more heat. In this case, the forward reaction is exothermic as indicated by a negative enthalpy change (ΔHο=-200 kJ). Therefore, a lower temperature would favor the forward reaction to produce more SO3.
Regarding pressure, according to the reaction, there are no gas molecules changing volume; thus, the pressure change will have no effect on the equilibrium.
Based on this analysis, the answer is option A. Low temperature and low pressure conditions will produce the greatest amount of SO3, as a lower temperature favors the exothermic reaction to produce more SO3, while pressure has no effect on the equilibrium.