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Bonus Question: Arrange Gas Samples by Pressure Consider the following gas samples at the same temperature. Arrange them from lowest to highest pressure. Since temperature is constant, we use Boyle's Law, which states that pressure is inversely proportional to volume if the number of particles is the same. However, if the volume is constant, the pressure increases with the number of gas molecules. Step 1: Count Gas Particles in Each Box ⚫ i: 3 Ne • ii: 4 Ne • iii: 5 Ne • iv: 7 Ne . v: 3 Ar • vi: 4 Ar . • vii: 7 Ar • viii: 8 Ar Step 2: Order by Pressure At constant temperature and volume, more gas particles mean higher pressure. Ordering from lowest to highest pressure: i = v < ii = vi < iii < vii = iv < viii Final Answer: i = v < ii = vi < iii < vii = iv < viii Final Summary of Answers: 1. Total volume of gas needed to collect 0.750 g of Ne: 0.91 L 2. Order of gas samples from lowest to highest pressure: i = v < ii = vi < iii < vii = iv < viii Question 8: Neon gas is collected over ethanol at 30°C under a total pressure of 1.10 atm. What total volume of gas must be gathered to obtain 0.750 g of neon? ⚫ Given: Mass of Ne = 0.750 g • Total pressure = 1.10 atm ⚫ Vapor pressure of ethanol = 30.2 torr ⚫ Molar mass of Ne = 20.1797 g/mol = • Temperature 30°C Convert to Kelvin: T 30+273.15 = 303.15 K Gas constant R = 0.0821 L-atm/mol.K Step 1: Convert Vapor Pressure of Ethanol to atm Since the total pressure includes the ethanol vapor pressure, we first convert it from torr to atm: Pethanol = 30.2 x 1 atm 760 torr = 0.0397 atm The pressure exerted by neon gas is: PNe = Ptotal - Pethanol PNe = 1.10 0.0397 1.0603 atm Step 2: Determine the Number of Moles of Neon n = mass molar mass 0.750 n 20.1797 n = 0.0372 mol Step 3: Use the Ideal Gas Law to Find Volume nRT V Р (0.0372) (0.0821) (303.15) V 1.0603 0.926 V = 0.907 L 1.0603 Final Answer: The total volume of gas required to obtain 0.750 g of Ne is 0.91 L.

Bonus Question: Arrange Gas Samples by Pressure Consider the following gas samples at the same temperature. Arrange them from lowest to highest pressure. Since temperature is constant, we use Boyle's Law, which states that pressure is inversely proportional to volume if the number of particles is the same. However, if the volume is constant, the pressure increases with the number of gas molecules. Step 1: Count Gas Particles in Each Box ⚫ i: 3 Ne • ii: 4 Ne • iii: 5 Ne • iv: 7 Ne . v: 3 Ar • vi: 4 Ar . • vii: 7 Ar • viii: 8 Ar Step 2: Order by Pressure At constant temperature and volume, more gas particles mean higher pressure. Ordering from lowest to highest pressure: i = v < ii = vi < iii < vii = iv < viii Final Answer: i = v < ii = vi < iii < vii = iv < viii Final Summary of Answers: 1. Total volume of gas needed to collect 0.750 g of Ne: 0.91 L 2. Order of gas samples from lowest to highest pressure: i = v < ii = vi < iii < vii = iv < viii Question 8: Neon gas is collected over ethanol at 30°C under a total pressure of 1.10 atm. What total volume of gas must be gathered to obtain 0.750 g of neon? ⚫ Given: Mass of Ne = 0.750 g • Total pressure = 1.10 atm ⚫ Vapor pressure of ethanol = 30.2 torr ⚫ Molar mass of Ne = 20.1797 g/mol = • Temperature 30°C Convert to Kelvin: T 30+273.15 = 303.15 K Gas constant R = 0.0821 L-atm/mol.K Step 1: Convert Vapor Pressure of Ethanol to atm Since the total pressure includes the ethanol vapor pressure, we first convert it from torr to atm: Pethanol = 30.2 x 1 atm 760 torr = 0.0397 atm The pressure exerted by neon gas is: PNe = Ptotal - Pethanol PNe = 1.10 0.0397 1.0603 atm Step 2: Determine the Number of Moles of Neon n = mass molar mass 0.750 n 20.1797 n = 0.0372 mol Step 3: Use the Ideal Gas Law to Find Volume nRT V Р (0.0372) (0.0821) (303.15) V 1.0603 0.926 V = 0.907 L 1.0603 Final Answer: The total volume of gas required to obtain 0.750 g of Ne is 0.91 L.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter5: The Gaseous State
Section: Chapter Questions
Problem 5.1QP
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Bonus Question: Arrange Gas Samples by Pressure Consider the following gas samples at the same temperature. Arrange them from lowest to highest pressure. Since temperature is constant, we use Boyle's Law, which states that pressure is inversely proportional to volume if the number of particles is the same. However, if the volume is constant, the pressure increases with the number of gas molecules. Step 1: Count Gas Particles in Each Box ⚫ i: 3 Ne • ii: 4 Ne • iii: 5 Ne • iv: 7 Ne . v: 3 Ar • vi: 4 Ar . • vii: 7 Ar • viii: 8 Ar Step 2: Order by Pressure At constant temperature and volume, more gas particles mean higher pressure. Ordering from lowest to highest pressure: i = v < ii = vi < iii < vii = iv < viii Final Answer: i = v < ii = vi < iii < vii = iv < viii Final Summary of Answers: 1. Total volume of gas needed to collect 0.750 g of Ne: 0.91 L 2. Order of gas samples from lowest to highest pressure: i = v < ii = vi < iii < vii = iv < viii
Transcribed Image Text:Bonus Question: Arrange Gas Samples by Pressure Consider the following gas samples at the same temperature. Arrange them from lowest to highest pressure. Since temperature is constant, we use Boyle's Law, which states that pressure is inversely proportional to volume if the number of particles is the same. However, if the volume is constant, the pressure increases with the number of gas molecules. Step 1: Count Gas Particles in Each Box ⚫ i: 3 Ne • ii: 4 Ne • iii: 5 Ne • iv: 7 Ne . v: 3 Ar • vi: 4 Ar . • vii: 7 Ar • viii: 8 Ar Step 2: Order by Pressure At constant temperature and volume, more gas particles mean higher pressure. Ordering from lowest to highest pressure: i = v < ii = vi < iii < vii = iv < viii Final Answer: i = v < ii = vi < iii < vii = iv < viii Final Summary of Answers: 1. Total volume of gas needed to collect 0.750 g of Ne: 0.91 L 2. Order of gas samples from lowest to highest pressure: i = v < ii = vi < iii < vii = iv < viii
Question 8: Neon gas is collected over ethanol at 30°C under a total pressure of 1.10 atm. What total volume of gas must be gathered to obtain 0.750 g of neon? ⚫ Given: Mass of Ne = 0.750 g • Total pressure = 1.10 atm ⚫ Vapor pressure of ethanol = 30.2 torr ⚫ Molar mass of Ne = 20.1797 g/mol = • Temperature 30°C Convert to Kelvin: T 30+273.15 = 303.15 K Gas constant R = 0.0821 L-atm/mol.K Step 1: Convert Vapor Pressure of Ethanol to atm Since the total pressure includes the ethanol vapor pressure, we first convert it from torr to atm: Pethanol = 30.2 x 1 atm 760 torr = 0.0397 atm The pressure exerted by neon gas is: PNe = Ptotal - Pethanol PNe = 1.10 0.0397 1.0603 atm Step 2: Determine the Number of Moles of Neon n = mass molar mass 0.750 n 20.1797 n = 0.0372 mol Step 3: Use the Ideal Gas Law to Find Volume nRT V Р (0.0372) (0.0821) (303.15) V 1.0603 0.926 V = 0.907 L 1.0603 Final Answer: The total volume of gas required to obtain 0.750 g of Ne is 0.91 L.
Transcribed Image Text:Question 8: Neon gas is collected over ethanol at 30°C under a total pressure of 1.10 atm. What total volume of gas must be gathered to obtain 0.750 g of neon? ⚫ Given: Mass of Ne = 0.750 g • Total pressure = 1.10 atm ⚫ Vapor pressure of ethanol = 30.2 torr ⚫ Molar mass of Ne = 20.1797 g/mol = • Temperature 30°C Convert to Kelvin: T 30+273.15 = 303.15 K Gas constant R = 0.0821 L-atm/mol.K Step 1: Convert Vapor Pressure of Ethanol to atm Since the total pressure includes the ethanol vapor pressure, we first convert it from torr to atm: Pethanol = 30.2 x 1 atm 760 torr = 0.0397 atm The pressure exerted by neon gas is: PNe = Ptotal - Pethanol PNe = 1.10 0.0397 1.0603 atm Step 2: Determine the Number of Moles of Neon n = mass molar mass 0.750 n 20.1797 n = 0.0372 mol Step 3: Use the Ideal Gas Law to Find Volume nRT V Р (0.0372) (0.0821) (303.15) V 1.0603 0.926 V = 0.907 L 1.0603 Final Answer: The total volume of gas required to obtain 0.750 g of Ne is 0.91 L.
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