An organic compound contains 21,20% carbon, 5,30% hydrogen and the rest is arsenic and oxygen. From 0,500 grams of that compound was obtained 0,802 grams of magnesium ammonium arsenate, MgNH
4AsO
4. Calculate the mass fraction of arsenic and oxygen in that organic compound and its empirical formula.
Solution: w(As)=66,30%, w(O)=7,20%, C4H12As2O_______________________________________________________________________________________________
My attempt:
w(As+O)=73,5%
C
aH
bAs
cO
d + X
MgNH
4AsO
4 + Y
M(C
aH
bAs
cO
d):M(MgNH
4AsO
4)= m(MgNH
4AsO
4):m(C
aH
bAs
cO
d)
M(C
aH
bAs
cO
d) = M(MgNH
4AsO
4)*m(MgNH
4AsO
4)/m(C
aH
bAs
cO
d)=290,741
N(C, C
aH
bAs
cO
d)=w(C, C
aH
bAs
cO
d)*M(C
aH
bAs
cO
d)/M(C)=4,846
N(H, C
aH
bAs
cO
d)=w(H, C
aH
bAs
cO
d)*M(C
aH
bAs
cO
d)/M(H)=15,257
I have no clue what should my proceeding step be, even though my calculations aren't correct.
Thank you in advance!