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0.22g sample of volatile compound,containing $C,H$ and $Cl$ only on combustion in $O_2$ gave 0.195g $CO_2$ and 0.0804g $H_2O$.If 0.120g of the compound occupied a volume of 37.24ml at $105^{\large\circ}$ and 768mm of pressure,calculate molecular formula of compound.


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Step 1:
$\large\frac{768}{760}$$\times \large\frac{37.24}{1000}=\large\frac{0.120}{m}$$\times 0.0821\times 378$
Let formula of compound be $C_aH_6Cl_2$
$C_aH_bCl_2+(a+\large\frac{b}{4})$$O_2\rightarrow aCO_2+\large\frac{b}{2}$$H_2O+\large\frac{z}{2}$$Cl_2$
$99g\Rightarrow 44ag\;CO_2$
$6.22g\Rightarrow \large\frac{44a\times 0.22}{99}$
$\therefore \large\frac{44a\times 0.22}{99}$$=0.195$
Step 2:
Similarly $0.22g$ compound gives =$\large\frac{18\times b\times 0.22}{2\times 99}$g $H_2O$
$\large\frac{18\times b\times 0.22}{2\times 99}$$=0.0804$
Now $C_aH_bCl_2$
$12\times a+b+35.5z=99$
$\therefore C_2H_4Cl_2$
Hence (b) is the correct answer.
answered Nov 6, 2013 by sreemathi.v

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