Question

1. 17.0 grams of xenon hexafluoride is in a solid container. How many milliliters of that gas

are in that container at 302.7°C and 821.4 Torr?

Answer 1

Answer: The volume of gas is 3020 ml

Step-by-step explanation:

According to ideal gas equation:

`PV=nRT`

P = pressure of gas = 821.4 torr = 1.08 atm (760 torr = 1atm)

V = Volume of gas in L = ?

n = number of moles =
`\frac{\text {given mass}}{\text {Molar mass}}=(17.0g)/(245.28g/mol)=0.069mol`

R = gas constant =
`0.0821Latm/Kmol`

T =temperature =
`302.7^0C=(302.7+273)K=575.7K`

`V=(nRT)/(P)`

`V=(0.069mol* 0.0821Latm/K mol* 575.7K)/(1.08atm)=3.02L=3020ml`

Thus volume of gas is 3020 ml