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 : - Sri Chaitanya Infinity Learn Best Online Courses for NCERT Solutions, CBSE, ICSE, JEE, NEET, Olympiad and Class 6 to 12

A
43 g
B
86 g
C
129 g
D
172 g

Solution:

Moles of $C = n_{{CO}_{2}} = \frac{2 .64}{44} = 0 .06$
$\Rightarrow mass of C = 0 .72$
Moles of H = 2 x moles of H₂O
$= 2 \times \frac{1 .26}{18} = 0 .14$
mass of H = 0.14
Compound does not contains oxygen,
So, $EF \to C_{0 .06} H_{0 .14} \Rightarrow C_{3} H_{7}$
Lowest M,M. = 43

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 :

Solution:

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