Question

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

Answer 1

Answer: The volume of gas is 3020 ml

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 = $\frac{\text {given mass}}{\text {Molar mass}}=\frac{17.0g}{245.28g/mol}=0.069mol$

R = gas constant =$0.0821Latm/Kmol$

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

$V=\frac{nRT}{P}$

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

Thus volume of gas is 3020 ml