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Ch.15 - Chemical Equilibrium
All textbooksTro 4th EditionCh.15 - Chemical EquilibriumProblem 83
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Chapter 15, Problem 83

Is Ammonia synthesized according to the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) with Kp = 5.3 * 10^-5 at 725K?

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1
Identify the reaction: \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \).
Understand that \( K_p \) is the equilibrium constant for the reaction in terms of partial pressures, given as \( 5.3 \times 10^{-5} \) at 725K.
Write the expression for \( K_p \) for the reaction: \( K_p = \frac{{(P_{NH_3})^2}}{{(P_{N_2})(P_{H_2})^3}} \).
Determine the partial pressures of \( N_2 \), \( H_2 \), and \( NH_3 \) at equilibrium if not provided, or assume initial conditions to calculate them.
Substitute the partial pressures into the \( K_p \) expression to check if the calculated \( K_p \) matches the given \( 5.3 \times 10^{-5} \).
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Textbook Question

Consider the endothermic reaction: C2H4(g) + I2(g) ⇌ C2H4I2(g) If you were trying to maximize the amount of C2H4I2 produced, which tactic might you try? Assume that the reaction mixture reaches equilibrium. a. decreasing the reaction volume b. removing I2 from the reaction mixture c. raising the reaction temperature d. adding C2H4 to the reaction mixture

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Textbook Question

Consider the reaction: H2(g) + I2(g) ⇌ 2 HI(g) A reaction mixture at equilibrium at 175 K contains PH2 = 0.958 atm, PI2 = 0.877 atm, and PHI = 0.020 atm. A second reaction mixture, also at 175 K, contains PH2 = PI2 = 0.621 atm and PHI = 0.101 atm. Is the second reaction at equilibrium? If not, what will be the partial pressure of HI when the reaction reaches equilibrium at 175 K?

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Open Question
Is the question asking for something specific about the reaction: 2 H2S(g) + SO2(g) ⇌ 3 S(s) + 2 H2O(g)?
Open Question
Is the question formulated correctly regarding the extraction of hydrogen from natural gas as per the given reaction CH4(g) + CO2(g) ⇌ 2 CO(g) + 2 H2(g) with Kp = 4.5 * 10^2 at 825K?
Textbook Question

A reaction vessel at 27 °C contains a mixture of SO2 (P = 3.00 atm) and O2 (P = 1.00 atm). When a catalyst is added, this reaction takes place: 2 SO2( g) + O2( g) ⇌ 2 SO3( g). At equilibrium, the total pressure is 3.75 atm. Find the value of Kc.

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Textbook Question

At 70 K, CCl4 decomposes to carbon and chlorine. The Kp for the decomposition is 0.76. Find the starting pressure of CCl4 at this temperature that will produce a total pressure of 1.0 atm at equilibrium.

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