Question #0ebb5

May 18, 2016

let us assume that we ave started with 100 g of compound and the compound on decomposition gives 67.62 g ( 67.62%) of Uranium and 32.38 g ( 32.38%) of fluorine.

Step II Calculate the number of moles of each element \

${n}_{U}$ = 67.62 g / 238 g $m o {l}^{-} 1$

${n}_{U}$ = 0.284 mol

${n}_{F}$ = 32.38 g / 19 g $m o {l}^{-} 1$

${n}_{F}$ = 1.70 mol

Step III ; Calculating the simple whole ratio

U = 0.284 / 0.284 = 1 and F = 1.70 / 0.284 = 6

the empirical formula is ${U}_{1}$ ${F}_{6}$ or U${F}_{6}$