Question

A 1.44-g sample of an unknown pure gas occupies a volume of 0.335 L at a pressure of and a temperature of 100.0°C. The unknown gas is ________.

Answer 1

Answer:

Xenon

Explanation:

Step 1: Given data

• Mass (m): 1.44 g

• Volume (V): 0.335 L

• Pressure (P): 1.00 atm (I looked it up)

• Temperature (T): 100.0°C

Step 2: Convert the temperature to Kelvin

K = °C + 273.15 = 100.0°C + 273.15 = 373.2 K

Step 3: Calculate the number of moles (n)

We will use the ideal gas equation.

P × V = n × R × T

n = P × V / R × T

n = 1.00 atm × 0.335 L / (0.0821 atm.L/mol.K) × 373.2 K

n = 0.0109 mol

Step 4: Calculate the molar mass of the gas

M = 1.44 g / 0.0109 mol = 132 g/mol

Step 5: Identify the gas

The gas with a molar mass of about 132 g/mol is xenon.

Answer 2

The gas with a molar mass of 132.11g/mol is Xenon. Hence the unknown gas is Xenon

Using the ideal gas equation

$PV=nRT\\n=\frac{PV}{RT}$

R is the Boltzmann constant = 8.31

V is the volume of the gas = 0.355L

P is the pressure = 1.00atm

T is the temperature of the gas = 100.0°C = 373K

To get the unknown gas, we need to first get the number of moles of gas:

$n=\frac{1.0\times 0.335}{0.0831 \times 373}\\n=0.0109 moles$

Get the molar mass of the element;

$n=\frac{m}{M}\\0.0109=\frac{1.44}{M}\\M=\frac{1.44}{0.0109}\\M= 132.11g/mol$

The gas with a molar mass of 132.11g/mol is Xenon. Hence the unknown gas is Xenon

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