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.
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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