1. Write down the chemical formula for butane and calculate its molar mass. 2. Derive the expression for the molar mass in terms of the mass, pressure, volume, and temperature of a gas (hint: use the ideal gas law and the definition of molar mass in Equation (2)). 3. Using Dalton’s law of partial pressures, calculate the total pressure of a mixture of three gases, N2, He, and Ne, at partial pressures of 0.32 atm for N2, 0.15 atm for He, and 0.42 atm for Ne that is in a 2.5 L flask at 15 ˚C.
1. Write down the chemical formula for butane and calculate its molar mass. 2. Derive the expression for the molar mass in terms of the mass, pressure, volume, and temperature of a gas (hint: use the ideal gas law and the definition of molar mass in Equation (2)). 3. Using Dalton’s law of partial pressures, calculate the total pressure of a mixture of three gases, N2, He, and Ne, at partial pressures of 0.32 atm for N2, 0.15 atm for He, and 0.42 atm for Ne that is in a 2.5 L flask at 15 ˚C.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter8: Properties Of Gases
Section8.7: Kinetic-molecular Theory And The Velocities Of Gas Molecules
Problem 8.12PSP
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1. Write down the chemical formula for butane and calculate its molar mass.
2. Derive the expression for the molar mass in terms of the mass, pressure, volume, and temperature of a gas (hint: use the
3. Using Dalton’s law of partial pressures, calculate the total pressure of a mixture of three gases, N2, He, and Ne, at partial pressures of 0.32 atm for N2, 0.15 atm for He, and 0.42 atm for Ne that is in a 2.5 L flask at 15 ˚C.
4. The barometric pressure is generally given in units of inHg. Convert inHg to atm. Recall that 2.54cm = 1inch. Use dimensional analysis.
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