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yan [13]
2 years ago
5

Calculate the mass of xenon difluoride gas with a volume of 0.223 L, pressure of 0.799 atm and temperature of 47.0 oC.

Chemistry
1 answer:
Greeley [361]2 years ago
8 0

The mass of the gases can be determined by the moles of the gas in the ideal equation. The mass of xenon difluoride at 0.799 atm is 0.011 gms.

<h3>What is an ideal gas equation?</h3>

An ideal gas equation gives the moles of the substance from the temperature, volume, and pressure of the gas. The ideal gas equation can be shown as:

n = PV ÷ RT

Here, n = mass ÷ molar mass

Given,

Volume of xenon difluoride (V) = 0.223 L

Pressure of xenon difluoride (P) = 0.799 atm

Temperature of xenon difluoride (T) = 320.15 Kelvin

Gas constant (R) = 8.314 J⋅K⁻¹⋅mol⁻¹

The moles of the gas is calculated as:

n = PV ÷ RT

= 0.223 × 0.799 ÷ 8.314 × 320.15

= 0.1781 ÷ 2661.72

= 6.69 × 10⁻⁵ moles

Mass is calculated as:

169.29 × 6.69 × 10⁻⁵ = 0.011 gm

Therefore, 0.011 gms is the mass of xenon difluoride.

Learn more about ideal gas here:

brainly.com/question/14189621

#SPJ1

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