A) \[{{C}_{6}}{{H}_{6}}\]
B) \[{{C}_{6}}{{H}_{12}}\]
C) \[{{C}_{8}}{{H}_{18}}\]
D) \[{{C}_{10}}{{H}_{6}}\]
Correct Answer: A
Solution :
[a] \[{{K}_{b}}=3.6K\,kg/mol.\] \[\Delta {{T}_{f}}=16.6-16.14=0.46{}^\circ C\] \[\Delta {{T}_{f}}=\frac{100{{k}_{f}}{{w}_{1}}}{{{m}_{1}}{{w}_{2}}}\] \[0.46=\frac{100\times 3.6\times 1}{{{m}_{1}}\times 100}\] \[{{m}_{1}}=\frac{36}{0.46}=78.26g\] \[C=\frac{92.3}{100}\times 78.26=72.23g\] \[H=\frac{7.7\times 78.26}{100}=6.026g\] Whole ratio \[C=\frac{72.23}{1}=6.02\] \[H=\frac{6.026}{1}=6.02\] Therefore, the molecular formula is \[{{C}_{6}}{{H}_{6.}}\]
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