Textbook Question
When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) (a) Calculate Kc for this reaction at this temperature.
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Ch.15 - Chemical Equilibrium
Chapter 15, Problem 76b
A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br2(𝑔) An equilibrium mixture in a 5.00-L vessel at 100°C contains 3.22 g of NOBr, 2.46 g of NO, and 6.55 g of Br2. (b) What is the total pressure exerted by the mixture of gases?
Verified step by step guidance1
Determine the molar masses of NOBr, NO, and Br_2 using the periodic table.
Convert the given masses of NOBr, NO, and Br_2 to moles by dividing each mass by its respective molar mass.
Use the ideal gas law, PV = nRT, to calculate the partial pressure of each gas. Here, P is the pressure, V is the volume (5.00 L), n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin (convert 100°C to Kelvin by adding 273.15).
Calculate the partial pressure for each gas: P_NOBr, P_NO, and P_Br2.
Sum the partial pressures of NOBr, NO, and Br_2 to find the total pressure exerted by the mixture of gases.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ideal Gas Law
The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the total pressure of a gas mixture, as it allows us to determine how the quantities of gases present affect the overall pressure in a given volume.
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Ideal Gas Law Formula
Molar Mass and Mass to Moles Conversion
To find the total pressure exerted by the gas mixture, it is necessary to convert the mass of each gas into moles using their respective molar masses. This conversion is crucial because the Ideal Gas Law requires the number of moles (n) to calculate pressure, making it a fundamental step in solving the problem.
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01:29Mass and Moles Conversion
Dalton's Law of Partial Pressures
Dalton's Law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas. This principle is important for determining the total pressure in the vessel, as it allows us to calculate the contribution of each gas based on its mole fraction and the total number of moles present.
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00:27Dalton's Law and Partial Pressure
Related Practice
Textbook Question
When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) (c) According to Le Châtelier's principle, would the percent of SO2Cl2 that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?
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Textbook Question
A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br2(𝑔) An equilibrium mixture in a 5.00-L vessel at 100°C contains 3.22 g of NOBr, 2.46 g of NO, and 6.55 g of Br2. (c) What was the mass of the original sample of NOBr?
Textbook Question
Consider the hypothetical reaction A(𝑔) ⇌ 2 B(𝑔). A flask is charged with 0.75 atm of pure A, after which it is allowed to reach equilibrium at 0°C. At equilibrium, the partial pressure of A is 0.36 atm. (c) To maximize the yield of product B, would you make the reaction flask larger or smaller?
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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