We're being asked to determine which condition will maximize the partial pressure of CO(g). We're given the following reaction at equilibrium:
2 CO2 (g) ⇌ 2 CO (g) + O2 (g) ΔH° = -514 kJ
We're going to use Le Chatelier's Principle to determine the right conditions.
Since the reaction is exothermic, ΔH = (–), heat is given off as a product:
2 CO2 (g) ⇌ 2 CO (g) + O2 (g) + heat
Consider the following reaction at equilibrium:
2CO2 (g) ⇌ 2CO (g) + O2 (g) ΔH° = -514 kJ
Le Chatelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction __________.
a. at high temperature and high pressure
b. at high temperature and low pressure
c. at low temperature and low pressure
d. at low temperature and high pressure
e. in the presence of solid carbon
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Le Chatelier's Principle concept. You can view video lessons to learn Le Chatelier's Principle . Or if you need more Le Chatelier's Principle practice, you can also practice Le Chatelier's Principle practice problems.
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Based on our data, we think this problem is relevant for Professor Mccurdy's class at UCD.