Answer:
Molecular formula for the compound is: C₄H₁₀
Explanation:
We analyse the data given.
82.76% means, that in 100g of compound 82.76 g are C
We have the molar mass which is 58.1 g/mol, so let's determine the mass of C, and then, its moles. Therefore we make this rule of three:
In 100 g of compound we have 82.76 g of C
In 58.1 g of compound we may have (85.1 . 82.76) / 100 = 48 g of C
If we convert the mass to moles: 48 g . 1mol / 12g = 4 moles of C
we notice that the compound has 4 moles of C
Molar mass of compound is 58.1 g/mol
48 g of compound are C, therefore (58 - 48) = 10 g are from H
If we convert the mass to moles → 10 g . 1 mol/1 g = 10 moles
Molecular formula for the compound is: C₄H₁₀
Notice: Centesimal composition for H in the compound
(10g / 58 g) . 100 = 17.24 %
17.24 % + 82.76% = 100%
Answer:
C4H10.
Explanation:
The % of Hydrogen = 100 - 82.76 = 17.24%
Dividing by the atomic masses
C = 82.76 / 12.011 = 6.89
H = 17.24 / 1.008 = 17.1
C: H = 1:2.48
= 2:5
So the empirical formula is C2H5 = 2*12.011+ 5.04 = 29.05 g
Now the molecular mass is 58.1 g which is 2 * 29.05 so the molecular formula is
2 * (C2H5) = C4H10.
