What is the answer to this Chemisty problem?

Question

water is added to 4.267 grams of UF6. the only products are 3.73 grams of a solid containing only uranium, oxygen and flourine and .970 of a gas. The gas is 95% flourine and the remainder is hydrogen.


a. what is the empirical formula of the gas?
b. what fraction of the flouriine of the original compound is in the solid and what fraction in the gas after the reaction?
c. what is the formula of the solid product?
d. write a balenced equation for the reaction between UF6 and H20 , assume that the empirical formula of he gas is the true fromula.

Answer 1

a) HF (hydrogen fluoride)

b) Of the 4.267 grams of UF6, 1.383 grams of F and 2,884 grams of U. (This was calculated from 6 * atomic mass of F / formula mass of UF6).

fraction in HF = 0.95(0.970 grams)/1.383 grams (= about 2/3)

c) UO2F2

d) 2H20 + UF6 --> UO2F2 + 4HF

Answer 2

a. The empirical formula of the gas can be found as follows:

H5/1 F95/19

(Notice that i have divided the % of each element by its atomic mass, which will give you the mole ratio ie the empirical formula.)

b. Work out moles of UF6 in 4.267 g (hint; divide by its molecular mass). Notice that there are 6 moles of F per mole of UF6. Do the same with the gas

c. and d. Rather than deprive you of the satisfaction of solving these last two, i will leave it for you to solve after you work out a. and b. above.

If you need more help, please email me or re post.

Answer 3

C2H5OH + (9/2)O2 = 2CO2 + 3H2O from the equation, utilising ratios.. while a million mol of ethanol reacts, 2 moles of carbon-dioxide is produced while 8.3 moles of ethanol reacts, x moles of carbondioxide is produced consequently.. x = (8.3*2)/a million x = sixteen.6 moles. the final suited answer is C

Answer 4

Richard , is right in his answer , good job