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Ch.15 - Chemical Equilibrium
All textbooksTro 4th EditionCh.15 - Chemical EquilibriumProblem 7
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Chapter 15, Problem 7

This reaction is exothermic. C6H12O6(s) + 6 O2(g) ⇌ 6 CO2(g) + 6 H2O(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?

Verified step by step guidance
1
Identify that the reaction is exothermic, meaning it releases heat as a product.
Apply Le Chatelier's Principle, which states that if a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance.
Consider the effect of increasing temperature: Since heat is a product in an exothermic reaction, increasing temperature adds more 'product', causing the equilibrium to shift to the left to consume the excess heat.
Consider the effect of decreasing temperature: Removing heat from the system will cause the equilibrium to shift to the right to produce more heat.
Understand that the equilibrium constant (K) for an exothermic reaction decreases with an increase in temperature, as the reaction shifts to the left, and increases with a decrease in temperature, as the reaction shifts to the right.
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Related Practice
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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Open Question
Nitrogen dioxide dimerizes according to the reaction: 2 NO2(g) ⇌ N2O4(g) Kp = 6.7 at 298 K. A 2.25-L container contains 0.055 mol of NO2 and 0.082 mol of N2O4 at 298 K. Is the reaction at equilibrium? If not, in which direction will the reaction proceed?
Open Question
Consider the reaction: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Kp = 0.0611 at 2000 K. A reaction mixture initially contains a CO partial pressure of 1344 torr and a H2O partial pressure of 1766 torr at 2000 K. Calculate the equilibrium partial pressures of each of the products.
Textbook Question

Write an expression for the equilibrium constant of each chemical equation.

a. SbCl5(g) ⇌ SbCl3(g) + Cl2(g)

b.2 BrNO(g) ⇌ 2 NO(g) + Br2(g)

c. CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g)

d. 2 CO(g) + O2(g) ⇌ 2 CO2(g)

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Textbook Question

Find and fix each mistake in the equilibrium constant expressions. a. 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = [H2][S2]/[H2S]

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Textbook Question

Find and fix each mistake in the equilibrium constant expressions. b. CO(g) + Cl2(g) ⇌ COCl2(g) K = [CO][Cl2]/[COCl2]

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