In 1811,Avogadro calculated the formula of ca | vedclass

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(B) Using the ideal gas equation: $PV = nRT = \frac{m}{M}RT$,where $M$ is the molar mass and $d = \frac{m}{V}$ is the density.The formula for molar ma

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$C_{10}H_{16}O$

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(B) Using the ideal gas equation: $PV = nRT = \frac{m}{M}RT$,where $M$ is the molar mass and $d = \frac{m}{V}$ is the density.The formula for molar mass is $M = \frac{dRT}{P}$.Given: $d = 3.84 \ g/L$,$R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$,$T = 210 + 273 = 483 \ K$,and $P = 1 \ atm$.Substituting the values: $M = \frac{3.84 	imes 0.0821 	imes 483}{1} \approx 152.2 \ g/mol$.Calculating the molar mass for the options:$A: C_{10}H_{14}O = (10 	imes 12) + (14 	imes 1) + 16 = 150 \ g/mol$$B: C_{10}H_{16}O = (10 	imes 12) + (16 	imes 1) + 16 = 152 \ g/mol$$C: C_{10}H_{16}O_2 = (10 	imes 12) + (16 	imes 1) + 32 = 168 \ g/mol$$D: C_{10}H_{18}O = (10 	imes 12) + (18 	imes 1) + 16 = 154 \ g/mol$Since the calculated molar mass is $152 \ g/mol$,the correct formula is $C_{10}H_{16}O$.

In $1811$,Avogadro calculated the formula of camphor by measuring the density of its vapour. Avogadro found the density to be $3.84 \ g/L$,when he made the measurement at $210 \ ^oC$ and $1 \ atm$ pressure. Which of the following is the correct formula of camphor?

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