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Ch.15 - Chemical Equilibrium
All textbooksBrown 14th EditionCh.15 - Chemical EquilibriumProblem 81
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Chapter 15, Problem 81

Solid NH4SH is introduced into an evacuated flask at 24 _x001F_C. The following reaction takes place: NH4SH(s) ⇌ NH3(g) + H2S(g). At equilibrium, the total pressure (for NH3 and H2S taken together) is 0.614 atm. What is Kp for this equilibrium at 24 _x001F_C?

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1
Identify the equilibrium reaction: NH4SH(s) ⇌ NH3(g) + H2S(g). Note that NH4SH is a solid and does not appear in the expression for Kp.
Write the expression for the equilibrium constant Kp for the reaction: Kp = P(NH3) * P(H2S), where P(NH3) and P(H2S) are the partial pressures of NH3 and H2S, respectively.
Recognize that at equilibrium, the total pressure is the sum of the partial pressures of NH3 and H2S: P(total) = P(NH3) + P(H2S) = 0.614 atm.
Assume that the partial pressures of NH3 and H2S are equal at equilibrium due to the stoichiometry of the reaction (1:1 ratio). Therefore, let P(NH3) = P(H2S) = x atm.
Set up the equation for total pressure: x + x = 0.614 atm, solve for x to find the partial pressures, and then substitute back into the Kp expression to find Kp.
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Textbook Question

As shown in Table 15.2, the equilibrium constant for the reaction N2(𝑔) + 3 H2(𝑔) ⇌ 2 NH3(𝑔) is 𝐾𝑝 = 4.34×10−3 at 300°C. Pure NH3 is placed in a 1.00-L flask and allowed to reach equilibrium at this temperature. There are 1.05 g NH3 in the equilibrium mixture. (b) What was the initial mass of ammonia placed in the vessel?

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Open Question
For the equilibrium 2 IBr(g) ⇌ I2(g) + Br2(g), Kp = 8.5 * 10^-3 at 150 _x001F_C. If 0.025 atm of IBr is placed in a 2.0-L container, what is the partial pressure of all substances after equilibrium is reached?
Textbook Question

For the equilibrium PH3BCl3(𝑠) ⇌ PH3(𝑔) + BCl3(𝑔) 𝐾𝑝 = 0.052 at 60 °C. (b) After 3.00 g of solid PH3BCl3 is added to a closed 1.500-L vessel at 60 °C, the vessel is charged with 0.0500 g of BCl3(𝑔). What is the equilibrium concentration of PH3?

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Textbook Question

A 0.831-g sample of SO3 is placed in a 1.00-L container and heated to 1100 K. The SO3 decomposes to SO2 and O2: 2SO3(𝑔) ⇌ 2 SO2(𝑔) + O2(𝑔) At equilibrium, the total pressure in the container is 1.300 atm. Find the values of 𝐾𝑝 and 𝐾𝑐 for this reaction at 1100 K.

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Textbook Question

Nitric oxide (NO) reacts readily with chlorine gas as follows: 2 NO(𝑔) + Cl2(𝑔) ⇌ 2 NOCl(𝑔) At 700 K, the equilibrium constant Kp for this reaction is 0.26. Predict the behavior of each of the following mixtures at this temperature and indicate whether or not the mixtures are at equilibrium. If not, state whether the mixture will need to produce more products or reactants to reach equilibrium. (b) PNO = 0.12 atm, PCl2 = 0.10 atm, PNOCl = 0.050 atm

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Textbook Question

At 900 °C, 𝐾𝑐 = 0.0108 for the reaction

CaCO3(𝑠) ⇌ CaO(𝑠) + CO2(𝑔)

A mixture of CaCO3, CaO, and CO2 is placed in a 10.0-L vessel at 900°C. For the following mixtures, will the amount of CaCO3 increase, decrease, or remain the same as the system approaches equilibrium?

(c) 30.5 g CaCO3, 25.5 g CaO, and 6.48 g CO2

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