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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?

User Vishy
by
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1 Answer

2 votes

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

User Salminnella
by
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