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A solution of $3.0 \times 10^{–4}$ kg of camphor ($C_{10}H_{16}O$) in $25.3 \times 10^{–3}$ kg of chloroform boils at 61.3$^{\large\circ}$C. If the boiling point of chloroform is 61.0$^{\large\circ}$C, calculate $K_b$ and $\Delta H_{vap}$ of chloroform.

1 Answer

36.7KJ/ml
Hence (A) is the correct answer.
answered Jun 12, 2014 by sreemathi.v
 

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