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The molar mass of a gas is determined as in the experiment described in experiment 8. The mass is determined to be 2. 01 g. The volume of the water, which is equal to the volume of the gas, is measured to be 243 ml, the boiling water temperature was 99. 8°c and the barometric pressure was 755 mm hg. Calculate the molar mass of the gas. Use 0. 0821 l·atm/mol·k as the value of the ideal gas law constant, r. Enter the value of your answer only. The value you enter should be expressed in g/mol.



Answer :

As in the experiment, a gas's molar mass is established. It is calculated that the mass is 2. 01 g, or 254 g/mol.

Explain what an ideal gas is.

The definition of an ideal gas is a gas in which the volume of the molecules and the forces between the molecules are so minimal as to not affect the behavior of the gas.

V=243 mL and P=755 mmHg

T = 98.8 degrees

PV=nRTn =7.8910-3

Gas mass is 2.01 grams.

Molar Mass = Mass in Moles, or 254g/mol.

Why is gas known as ideal gas?

The phrase "ideal gas" describes a fictitious gas made up of molecules that adhere to the following principles: No attraction or repellence exists between the molecules of ideal gases.

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