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A 3.95 g sample of an unknown gas at 53 °C and 1.05 atm is stored in a 2.35 L flask. What is the density of the gas? density: What is the molar mass of the gas? molar mass: g/L g/mol

A 3.95 g sample of an unknown gas at 53 °C and 1.05 atm is stored in a 2.35 L flask. What is the density of the gas? density: What is the molar mass of the gas? molar mass: g/L g/mol

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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## Determining the Density and Molar Mass of an Unknown Gas **Given:** - Mass of gas sample: 3.95 g - Temperature: 53 °C (convert to Kelvin for calculations: 53 + 273.15 = 326.15 K) - Pressure: 1.05 atm - Volume of flask: 2.35 L ### What is the density of the gas? To find the density, use the formula: \[ \text{Density} = \frac{\text{mass}}{\text{volume}} \] **Input fields:** **Density:** [______________] g/L ### What is the molar mass of the gas? To find the molar mass, use the Ideal Gas Law: \[ PV = nRT \] where: - \(P\) is the pressure (1.05 atm), - \(V\) is the volume (2.35 L), - \(n\) is the number of moles, - \(R\) is the ideal gas constant (0.0821 L·atm/mol·K), - \(T\) is the temperature (326.15 K). From the Ideal Gas Law, first find the number of moles (\(n\)): \[ n = \frac{PV}{RT} \] Then, use the molar mass formula: \[ \text{Molar Mass} = \frac{\text{mass}}{\text{moles}} \] **Input fields:** **Molar Mass:** [______________] g/mol By filling in these calculations, one can determine the density and molar mass of the given unknown gas sample.
Transcribed Image Text:## Determining the Density and Molar Mass of an Unknown Gas **Given:** - Mass of gas sample: 3.95 g - Temperature: 53 °C (convert to Kelvin for calculations: 53 + 273.15 = 326.15 K) - Pressure: 1.05 atm - Volume of flask: 2.35 L ### What is the density of the gas? To find the density, use the formula: \[ \text{Density} = \frac{\text{mass}}{\text{volume}} \] **Input fields:** **Density:** [______________] g/L ### What is the molar mass of the gas? To find the molar mass, use the Ideal Gas Law: \[ PV = nRT \] where: - \(P\) is the pressure (1.05 atm), - \(V\) is the volume (2.35 L), - \(n\) is the number of moles, - \(R\) is the ideal gas constant (0.0821 L·atm/mol·K), - \(T\) is the temperature (326.15 K). From the Ideal Gas Law, first find the number of moles (\(n\)): \[ n = \frac{PV}{RT} \] Then, use the molar mass formula: \[ \text{Molar Mass} = \frac{\text{mass}}{\text{moles}} \] **Input fields:** **Molar Mass:** [______________] g/mol By filling in these calculations, one can determine the density and molar mass of the given unknown gas sample.
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