An organic compound was found to contain 10.15% Carbon, 0.84% Hydrogen & 88.98% Chlorine. Molar mass of the compound was found to be 120g/mol. What is the molecular formula of the compound?
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Answers
Answer:
=>. Find chorine’s percentage.
Cl= 100- (10.4+0.84) =100- 11.24= 88.76%Find the mass of teach components in grams:
carbon: 10.4% so 10.4g out of 100g of total mixture.
hydrogen: 0.84g
Chlorine: 88.76gfind the no. of moles of each (no. of moles= total mass/ atomic mass):
Carbon: 10.4/ 12 = 0.8
hydrogen: 0.84/1 = 0.84
Chlorine: 88.76/35= 2.5devide smallest mole vale by all mole values and write their ratio:
1:1:3 = C:H:ClWrite the respective values of ratio as subscrits of the chemical symbol:
C1H1Cl3 = CHCl3
SO CHCL3 IS THE EMPIRICAL FORMULA OF THE COMPOUND.Find the empirical formula mass:
Mass of C + Mass of H + Mass of 3 atoms of Cl= empirical formula mass
12+1+(3x35)= 118 uDivide the molecular mass (that is given in the question) with the empirical formula mass:
119.5/118 = 1.01 which is approximately 1Multiply all the subscripts of the empirical formula with the answer of the previous step (which is 1 in this case):
C(1x1)H(1x1)CL(3x1)= CHCl3
Hence, the molecular formula of the compound is CHCl3.
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