Question

A 7.456 g sample of UF6 is added to water. 6.53 g of a solid containing U, F and O and 1.69 g of a gas are formed. The gas is 5% H and 95% F by mass.
a. What is the empirical formula of the gas? In this case, the empirical formula is the same as the molecular formula (I got HF4)
b. What is the molecular formula of the solid?
c. Write a balanced equation for the reaction between UF6 and H2O.

Answer 1

Oops, I got HF for a.

Answer 2

I agree with HF, i think you know why but if you need to understand how to find empiricals i can explain that to you

Answer 3

gimmy a sec for the other two

Answer 4

is there no other information on the solid? if not then it would appear that the reaction equation is H2O + UF6 -> UF4O+2HF though i am basing that off of balancing alone and not actual bonding laws. i came up with this by saying that H2O+UF6 -> aUbFcOd + eHF where the lowercase letters are coefficients and subscripts

Answer 5

then you just solve and you should end up with UF4O + 2HF. let me check that with stoich... one more moment please

Answer 6

stoich says its closer to 2H2O + UF6 -> UF2O2 +4HF
since you asked 4 hours ago im not sure if you will come back, if you do, ask for any reasoning behind my answer.

Answer 7

Thanks, your answer makes sense.

Answer 8

But how can you prove that UF2O2 is the molecular formula, not just the empirical formula?

Answer 9

you cant know, they mentioned nothing of molar mass so its impossible to tell if its the molecular or just empirical. because its impossible to tell, assume that this answer is correct... btw its a pretty common question and all the other answers are the same soo ima go with that :D