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Question 3: A sealed flask at room temperature contains a mixture of neon (Ne) and nitrogen (N2) gases. Ne has a mass of 3.25 g and exerts a pressure of 48.2 torr. . N2 contributes a pressure of 142 torr. • What is the mass of the N2 in the flask? • Atomic mass of Ne = 20.1797 g/mol • Atomic mass of N = 14.0067 g/mol Solution: We will use the Ideal Gas Law to determine the number of moles of each gas and calculate the mass of N2. PV = nRT where: • P = total pressure • V volume of the flask (same for both gases) n = number of moles of gas • R 0.0821 L atm/mol K • T = Room temperature (assume 298 K) Since both gases are in the same flask, their partial pressures correspond to their mole fractions. Step 1: Convert Pressures to Atmospheres 48.2 PNe = 0.0634 atm 760 142 PN2 = = 0.1868 atm 760 Step 2: Determine Moles of Ne nNe = mass molar mass 3.25 nNe 20.1797 nne 0.1611 mol Step 3: Use Partial Pressure Ratio to Find n Step 2: Determine Moles of Ne mass nNe molar mass 3.25 nNe = 20.1797 nNe =0.1611 mol Step 3: Use Partial Pressure Ratio to Find n N₂ Since pressure and moles are directly proportional, nNe PNe nN2 PN2 0.1611 0.0634 nN2 0.1868 0.1611 x 0.1868 NN2 = 0.0634 NN2 = 0.474 mol Step 4: Calculate Mass of N₂ Molar mass of N₂ = 2 × 14.0067 = 28.0134 g/mol. Mass of N2nN2 × MN2 Mass of N2 = (0.474)(28.0134) Mass of N2 = 13.28 g Final Answer: The mass of №2 in the flask is 13.28 g.

Question 3: A sealed flask at room temperature contains a mixture of neon (Ne) and nitrogen (N2) gases. Ne has a mass of 3.25 g and exerts a pressure of 48.2 torr. . N2 contributes a pressure of 142 torr. • What is the mass of the N2 in the flask? • Atomic mass of Ne = 20.1797 g/mol • Atomic mass of N = 14.0067 g/mol Solution: We will use the Ideal Gas Law to determine the number of moles of each gas and calculate the mass of N2. PV = nRT where: • P = total pressure • V volume of the flask (same for both gases) n = number of moles of gas • R 0.0821 L atm/mol K • T = Room temperature (assume 298 K) Since both gases are in the same flask, their partial pressures correspond to their mole fractions. Step 1: Convert Pressures to Atmospheres 48.2 PNe = 0.0634 atm 760 142 PN2 = = 0.1868 atm 760 Step 2: Determine Moles of Ne nNe = mass molar mass 3.25 nNe 20.1797 nne 0.1611 mol Step 3: Use Partial Pressure Ratio to Find n Step 2: Determine Moles of Ne mass nNe molar mass 3.25 nNe = 20.1797 nNe =0.1611 mol Step 3: Use Partial Pressure Ratio to Find n N₂ Since pressure and moles are directly proportional, nNe PNe nN2 PN2 0.1611 0.0634 nN2 0.1868 0.1611 x 0.1868 NN2 = 0.0634 NN2 = 0.474 mol Step 4: Calculate Mass of N₂ Molar mass of N₂ = 2 × 14.0067 = 28.0134 g/mol. Mass of N2nN2 × MN2 Mass of N2 = (0.474)(28.0134) Mass of N2 = 13.28 g Final Answer: The mass of №2 in the flask is 13.28 g.

Linear Algebra: A Modern Introduction
Linear Algebra: A Modern Introduction
4th Edition
ISBN:9781285463247
Author:David Poole
Publisher:David Poole
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Question 3: A sealed flask at room temperature contains a mixture of neon (Ne) and nitrogen (N2) gases. Ne has a mass of 3.25 g and exerts a pressure of 48.2 torr. . N2 contributes a pressure of 142 torr. • What is the mass of the N2 in the flask? • Atomic mass of Ne = 20.1797 g/mol • Atomic mass of N = 14.0067 g/mol Solution: We will use the Ideal Gas Law to determine the number of moles of each gas and calculate the mass of N2. PV = nRT where: • P = total pressure • V volume of the flask (same for both gases) n = number of moles of gas • R 0.0821 L atm/mol K • T = Room temperature (assume 298 K) Since both gases are in the same flask, their partial pressures correspond to their mole fractions. Step 1: Convert Pressures to Atmospheres 48.2 PNe = 0.0634 atm 760 142 PN2 = = 0.1868 atm 760 Step 2: Determine Moles of Ne nNe = mass molar mass 3.25 nNe 20.1797 nne 0.1611 mol Step 3: Use Partial Pressure Ratio to Find n
Transcribed Image Text:Question 3: A sealed flask at room temperature contains a mixture of neon (Ne) and nitrogen (N2) gases. Ne has a mass of 3.25 g and exerts a pressure of 48.2 torr. . N2 contributes a pressure of 142 torr. • What is the mass of the N2 in the flask? • Atomic mass of Ne = 20.1797 g/mol • Atomic mass of N = 14.0067 g/mol Solution: We will use the Ideal Gas Law to determine the number of moles of each gas and calculate the mass of N2. PV = nRT where: • P = total pressure • V volume of the flask (same for both gases) n = number of moles of gas • R 0.0821 L atm/mol K • T = Room temperature (assume 298 K) Since both gases are in the same flask, their partial pressures correspond to their mole fractions. Step 1: Convert Pressures to Atmospheres 48.2 PNe = 0.0634 atm 760 142 PN2 = = 0.1868 atm 760 Step 2: Determine Moles of Ne nNe = mass molar mass 3.25 nNe 20.1797 nne 0.1611 mol Step 3: Use Partial Pressure Ratio to Find n
Step 2: Determine Moles of Ne mass nNe molar mass 3.25 nNe = 20.1797 nNe =0.1611 mol Step 3: Use Partial Pressure Ratio to Find n N₂ Since pressure and moles are directly proportional, nNe PNe nN2 PN2 0.1611 0.0634 nN2 0.1868 0.1611 x 0.1868 NN2 = 0.0634 NN2 = 0.474 mol Step 4: Calculate Mass of N₂ Molar mass of N₂ = 2 × 14.0067 = 28.0134 g/mol. Mass of N2nN2 × MN2 Mass of N2 = (0.474)(28.0134) Mass of N2 = 13.28 g Final Answer: The mass of №2 in the flask is 13.28 g.
Transcribed Image Text:Step 2: Determine Moles of Ne mass nNe molar mass 3.25 nNe = 20.1797 nNe =0.1611 mol Step 3: Use Partial Pressure Ratio to Find n N₂ Since pressure and moles are directly proportional, nNe PNe nN2 PN2 0.1611 0.0634 nN2 0.1868 0.1611 x 0.1868 NN2 = 0.0634 NN2 = 0.474 mol Step 4: Calculate Mass of N₂ Molar mass of N₂ = 2 × 14.0067 = 28.0134 g/mol. Mass of N2nN2 × MN2 Mass of N2 = (0.474)(28.0134) Mass of N2 = 13.28 g Final Answer: The mass of №2 in the flask is 13.28 g.
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