Problem: Consider the following reaction at equilibrium:2CO2 (g) ⇌ 2CO (g) + O2 (g)     ΔH° = -514 kJLe 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 pressureb. at high temperature and low pressurec. at low temperature and low pressured. at low temperature and high pressuree. in the presence of solid carbon

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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


For temperature:

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Problem Details

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.