A 19.4 gram sample of gas is found to have a volume of 1.3 liters at 282 K and 1.2 atm. What is the molar mass of this gas? Show all of the work used to solve this problem.

Question

Chemistry

Brent Blankenship

27 February, 04:45

A 19.4 gram sample of gas is found to have a volume of 1.3 liters at 282 K and 1.2 atm. What is the molar mass of this gas? Show all of the work used to solve this problem.

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Answers (1)

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Aspen Garrett · Answer 1

Molar mass of the given gas can be calculated by using the ideal gas law, which is in the formula;

PV=nRT where P is pressure, V=volume, n = no. of moles, R=ideal gas constant, and T=temperature. This equation has to be dimensionally homogeneous. Use R=0.08206 L-atm/mol-K.

PV=nRT

(1.2 atm) (1.3 L) = n (0.08206) (282K)

n=0.0674 mol

In order to find the molar mass, divide the given mass with the obtained number of moles,

19.4 g/0.0674 mol = 287.78 g/mol