A mixture contained no flourine compound except methyl fluoroacetate, FCH2COOCH3 (molar mass- 92.1 g/mol). When chemically treated, all the flourine was converted to CaF2 (molar mass= 78.1 g/mol) The mass of CaF2 obtained was 32.4 g. Find the mass of methyl fluoroacetate in the original mixture.
2006-11-29 02:27:56 · 2 answers · asked by Kenneth B 1 in Science & Mathematics ➔ Chemistry
number of moles of Ca F2 obtained is 32.4/78.1 =0.415moles
you noticed that Ca F2 has 2 atoms fluorine and your compoun only one, so to obtain 0.415 moles, you must use 0.415*2 =0.83 moles
of FCH2COOCH3
to solve your problem multiply 0.83*92.1 =76.4 g
There Was 76.4 g in the mixture
2006-11-29 02:36:06 · answer #1 · answered by maussy 7 · 0⤊ 0⤋
Use the dimensional analysis technique:
32.4g CaF2 (1mol CaF2/78.1g CaF2)(2mol FOAc/1mol CaF2)(92.1g FOAc/1mol) = 76.4 g FOAc.
Where FOAc is fluoroacetate. Note ratio of 1:2 (F in starting material to product).
2006-11-29 02:39:27 · answer #2 · answered by Peter B 3 · 0⤊ 0⤋