Question

A number of compounds containing the heavier noble gases, and especially xenon, have been prepared. One of these is xenon hexafluoride (XeF6), which can be prepared by heating a mixture of xenon and fluorine gases. XeF6 is a white crystalline solid at room temperature and melts at about 325 K. A mixture of 0.0600 g of Xe and 0.0310 g of F2 is sealed into a 100.0-mL bulb. The bulb contains no air or other gases. The bulb is heated, and the reaction above goes to completion. Then, the sealed bulb is cooled back to 20.0°C. What will be the final pressure in the bulb, expressed in torr?

Answer 1

Answer:

The answer is "82.2 torr"

Explanation:

moles of Xe:

$= \frac{0.06}{131.293} \\\\ =0.00045699313 \ \mol$

moles of $F_2$:

$= \frac{0.0274}{38} \\\\= 0.00072105263\ \ mol$

moles of produced $XeF_2:$

$= 0.00024$

moles of left $Xe$:

$= 0.00021$

Calculate the Pressure:

$= \frac{(0.08206\times 0.00024 \times 293)}{(.1)} + \frac{(0.08206\times 0.00021 \times 293)}{(.1)} \\\\= 0.10819611 \ \ atm \\\\ = 0.10819611 \times 760 \\\\ = 82.2 \ \ torr$