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A 1.43-g sample of an unknown gas has a volume of 804 mL and a pressure of 852 mmHg at 59.0 °C. Calculate the molar mass of this compound.

A 1.43-g sample of an unknown gas has a volume of 804 mL and a pressure of 852 mmHg at 59.0 °C. Calculate the molar mass of this compound.

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 1.43-g sample of an unknown gas has a volume of 804 mL and a pressure of 852 mmHg at 59.0 °C. Calculate the molar mass of this compound. Approach g/mol The ideal gas law contains four variables (P. V. n, and T) and a constant (R = 0.082057 L atm/K mol): PV = nRT If you know three of the four variables, you can calculate the fourth. All properties must have units that match those in the gas constant: volume in liters, pressure in atmospheres, temperature in kelvins, and amount in moles. In this case you can solve for the amount (mol) of gas, n. Once n is determined, the molar mass is calculated by dividing the mass by the amount (mol) of gas.
Transcribed Image Text:A 1.43-g sample of an unknown gas has a volume of 804 mL and a pressure of 852 mmHg at 59.0 °C. Calculate the molar mass of this compound. Approach g/mol The ideal gas law contains four variables (P. V. n, and T) and a constant (R = 0.082057 L atm/K mol): PV = nRT If you know three of the four variables, you can calculate the fourth. All properties must have units that match those in the gas constant: volume in liters, pressure in atmospheres, temperature in kelvins, and amount in moles. In this case you can solve for the amount (mol) of gas, n. Once n is determined, the molar mass is calculated by dividing the mass by the amount (mol) of gas.
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