let in compound number of moles of C, H and O be x, y and z respectively
Number of moles of CO2 = mass of CO2 / molar mass CO2
= 23.7/44
= 0.5386
Number of moles of H2O = mass of H2O / molar mass H2O
= 4.85/18
= 0.2694
Since 1 mol of CO2 has 1 mol of C
Number of moles of C in CO2= 0.5386
so, x = 0.5386
Since 1 mol of H2O has 2 mol of H
Number of moles of H = 2*0.2694 = 0.5389
Molar mass of O = 16 g/mol
mass O = total mass - mass of C and H
= 7.0 - 0.5386*12 - 0.5389*1
= -2.525*10^-3
Since this is negative, there is no oxygen present.
Divide by smallest to get simplest whole number ratio:
C: 0.5386/0.5386 = 1
H: 0.5389/0.5386 = 1
So empirical formula is:CH
Molar mass of CH,
MM = 1*MM(C) + 1*MM(H)
= 1*12.01 + 1*1.008
= 13.018 g/mol
Now we have:
Molar mass = 26.0 g/mol
Empirical formula mass = 13.018 g/mol
Multiplying factor = molar mass / empirical formula mass
= 26.0/13.018
= 2
So molecular formula is:C2H2
Answer: C2H2
7.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar...
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