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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?

Sagot :

Answer: The volume of gas is 3020 ml

Explanation:

According to ideal gas equation:

[tex]PV=nRT[/tex]

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

V = Volume of gas in L = ?

n = number of moles = [tex]\frac{\text {given mass}}{\text {Molar mass}}=\frac{17.0g}{245.28g/mol}=0.069mol[/tex]

R = gas constant =[tex]0.0821Latm/Kmol[/tex]

T =temperature =[tex]302.7^0C=(302.7+273)K=575.7K[/tex]

[tex]V=\frac{nRT}{P}[/tex]

[tex]V=\frac{0.069mol\times 0.0821Latm/K mol\times 575.7K}{1.08atm}=3.02L=3020ml[/tex]

Thus volume of gas is 3020 ml

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