Complete combustion of 0.86 g of compound X gives 2.64 g of CO2 and 1.26 g of H2O. The lowest molecular mass X can have :

# Complete combustion of 0.86 g of compound X gives 2.64 g of CO2 and 1.26 g of H2O. The lowest molecular mass X can have :

1. A

43 g

2. B

86 g

3. C

129 g

4. D

172 g

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### Solution:

Moles of $\mathrm{C}={\mathrm{n}}_{{\mathrm{CO}}_{2}}=\frac{2.64}{44}=0.06$

Moles of H = 2 x moles of H2O
$=2×\frac{1.26}{18}=0.14$
mass of H = 0.14
Compound does not contains oxygen,
So, $\mathrm{EF}\to {\mathrm{C}}_{0.06}{\mathrm{H}}_{0.14}⇒{\mathrm{C}}_{3}{\mathrm{H}}_{7}$
Lowest M,M. = 43

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