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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.15 - Chemical EquilibriumProblema 76b
Capitolo 15, Problema 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, 3.08 g of NO, and 4.19 g of Br2. (b) What is the total pressure exerted by the mixture of gases?

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Calculate the number of moles of each gas present in the mixture using the formula: number of moles (n) = mass (g) / molar mass (g/mol). The molar masses are: NOBr = 106.92 g/mol, NO = 30.01 g/mol, Br2 = 159.808 g/mol.
Use the ideal gas law to find the total number of moles of gas in the vessel. The ideal gas law is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.
Calculate the total pressure using the ideal gas law rearranged to solve for P: P = (nRT) / V. Substitute the total number of moles calculated, the gas constant, the temperature in Kelvin, and the volume of the vessel.
Ensure all units are consistent when substituting values into the ideal gas law equation to calculate the pressure in atmospheres.

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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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02:28
Mass 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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00:27
Dalton's Law and Partial Pressure
Pratica correlata
Domanda del libro di testo

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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Domanda del libro di testo

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, 3.08 g of NO, and 4.19 g of Br2. (c) What was the mass of the original sample of NOBr?

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