A) \[256\,g\,mo{{l}^{-1}}\]
B) \[2.56\,g\,mo{{l}^{-1}}\]
C) \[512\times {{10}^{3}}\,g\,mo{{l}^{-1}}\]
D) \[2.56\times {{10}^{4}}\,g\,mo{{l}^{-1}}\]
Correct Answer: A
Solution :
By using, \[m=\frac{{{K}_{f}}\times 1000\times w}{\Delta {{T}_{f}}\times {{W}_{\text{Solvent}\,}}(gm)}\]\[=\frac{5.12\,\times 1000\times 1}{0.40\times 50}\] \[=256\,gm/mol\] Hence, molecular mass of the solute \[=256\,gm\,mo{{l}^{-1}}\]
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