Question

Part 1. Determine the molar mass of a 0.622-gram sample of gas having a volume of 2.4 L at 287 K and 0.850 atm. Show your work.

Answer 1

If a sample of gas is a 0.622-gram, volume of 2.4 L at 287 K and 0.850 atm. Then the molar mass of the gas is 7.18.

What is an ideal gas equation?

The ideal gas equation is given below.

$PV = nRT$

The equation can be written as

$\rm PV = \dfrac{m}{M} \ RT\\\\\\MPV = mRT$

Where M is the molar mass, P is the pressure, V is the volume, R is the universal gas constant, T is the temperature, and m is the mass of the gas.

Then the molar mass of a 0.622-gram sample of gas has a volume of 2.4 L at 287 K and 0.850 atm.

V = 2.4 L = 0.0024

P = 0.85 atm = 86126.25 Pa

T = 287 K

m = 0.622

R = 8.314

Then we have

$\begin{aligned} \rm M \times 86126.25 \times 0.0024&= 0.622 \times 8.314 \times 287\\\\\rm M &= 7.18 \end{aligned}$

Then the molar mass of the gas is 7.18.

More about the ideal gas equation link is given below.

brainly.com/question/4147359

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