A sample of a compound contains 60.0 g C and 5.05 g H. Its molar mass is 78.12 g/mol. What is the compound’s molecular formula?
CH C2H2 C6H6 C6H
2 answers:
A sample of a compound contains 60.0 g C and 5.05 g H.
divide by molar mass of C(12) and H(1) to get molar ratio
C: 60/12=5 and H: 5/1=5
so C:H=5:5=1:1
total molar mass=78
divide by 1C+1H to find the formula: 78/(12+1)=78/13=6
compound is C6H6
Step 1: Calculate Moles for each Element:
Mole of C = 60.0 / 12 = 5
Mole of H = 5.05 / 1.008 = 5.009
Step 2: Calculate Mole Ratio:
Divide each mole value with least mole value.
H : C
5.009/5 : 5/5
1 : 1
So,
Empirical Formula = C₁H₁ or CnHn ------ (1)
Step 3: Calculate Molecular Formula:
By using formula,
n = Molecular Mass / Empirical Formula Mass
Molecular Mass = 78.12 g/mol
Empirical Formula Mass = 12 + 1 = 13 ∴ C = 12 & H = 1
So,
n = 78.12 / 13
n = 6
Putting value of n in eq. 1,
C₆H₆
Result:
The correct answer is C₆H₆.
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