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Ch.16 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.16 - Chemical EquilibriumProblem 75c
Chapter 16, Problem 75c

Coal, which is primarily carbon, can be converted to natural gas, primarily CH4, by the exothermic reaction: C(s) + 2 H2(g) ⇌ CH4(g) Which disturbance will favor CH4 at equilibrium? c. raising the temperature of the reaction mixture

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1
Identify the type of reaction: The given reaction C(s) + 2 H2(g) ⇌ CH4(g) is an exothermic reaction, meaning it releases heat.
Apply Le Chatelier's Principle: According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change, the system will adjust itself to counteract that change and restore a new equilibrium.
Analyze the effect of temperature: Increasing the temperature of an exothermic reaction adds heat to the system.
Predict the shift in equilibrium: Adding heat to an exothermic reaction will shift the equilibrium towards the reactants according to Le Chatelier's Principle.
Conclude the effect on CH4 production: Raising the temperature of the reaction mixture will not favor the production of CH4; instead, it will favor the formation of the reactants, C(s) and H2(g).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. This principle helps predict how a system at equilibrium will respond to changes in concentration, temperature, or pressure, favoring the formation of products or reactants.
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Le Chatelier's Principle

Exothermic Reactions

An exothermic reaction is one that releases energy, usually in the form of heat, to the surroundings. In the given reaction, the formation of CH4 from carbon and hydrogen is exothermic, meaning that increasing the temperature will shift the equilibrium position to favor the reactants, as the system will try to absorb the added heat.
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Endothermic & Exothermic Reactions

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Changes in temperature can alter the value of K, influencing the position of equilibrium. For exothermic reactions, increasing temperature typically decreases K, favoring reactants over products.
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Related Practice
Textbook Question

Carbon monoxide replaces oxygen in oxygenated hemoglobin according to the reaction: HbO2(aq) + CO(aq) ⇌ HbCO(aq) + O2(aq) a. Use the reactions and associated equilibrium constants at body temperature given here to find the equilibrium constant for the reaction just shown. Hb(aq) + O2(aq) ⇌ HbO2(aq) Kc = 1.8 Hb(aq) + CO(aq) ⇌ HbCO(aq) Kc = 306

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Textbook Question

At 650 K, the reaction MgCO3(s) ⇌ MgO(s) + CO2(g) has Kp = 0.026. A 10.0-L container at 650 K has 1.0 g of MgO(s) and CO2 at P = 0.0260 atm. The container is then compressed to a volume of 0.100 L. Find the mass of MgCO3 that is formed.

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Textbook Question

Coal, which is primarily carbon, can be converted to natural gas, primarily CH4, by the exothermic reaction: C(s) + 2 H2(g) ⇌ CH4(g) Which disturbance will favor CH4 at equilibrium?

a. adding more C to the reaction mixture b. adding more H2 to the reaction mixture d. lowering the volume of the reaction mixture f. adding neon gas to the reaction mixture

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Textbook Question

Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. b. PCl3(g) + Cl2(g) ⇌ PCl5(g) (volume is increased)

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Textbook Question

This reaction is endothermic. C(s) + CO2(g) ⇌ 2 CO(g) Predict the effect (shift right, shift left, or no effect) of increasing and decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature?

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