A chemist heats 26.26 g of xenon (131.3 g/mol) with fluorine at 573 K and 60 bar, and all the xenon…
Contributed by StemPy LabTry it on paper first. A hint, the key idea and the worked solution are here when you need them.
A chemist heats of xenon () with fluorine at and , and all the xenon turns into XeF6 (). Take the molar mass of F2 as . Find the mass of fluorine needed and the mass of XeF6 formed. Treat the fluorine as an ideal gas and find the volume that this mass of fluorine fills at and . Use .
Need a reminder? The key ideaShow
Xenon has 8 outer electrons, and each fluorine atom uses one of them. A double bond to oxygen counts as one region and uses 2 electrons. XeF2, XeF4 and XeF6 are made from Xe and F2 in the ratios 1 : 1, 1 : 2 and 1 : 3. The hydrolysis of XeF6 gives XeO3 and HF. In a disproportionation the same element is oxidised and reduced.
The worked solution
Have you tried it?
Work it out on paper first. It is fine to get stuck or make a mistake: that is how we learn. When you are ready, go through the solution one step at a time, and check each step against your own.
Step 1. Moles of xenon. .
Step 2. Fluorine. Three F2 for each Xe: , which is .
Step 3. Xenon hexafluoride. .
Step 4. Volume. . Then .
Answer: of fluorine, of XeF6 and .
Check. Mass is kept: . Real fluorine at 60 bar is not an ideal gas, so the true volume differs a little.
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