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.
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