A) \[{{C}_{5}}{{H}_{10}}\]
B) \[{{C}_{6}}{{H}_{12}}\]
C) \[{{C}_{4}}{{H}_{8}}\]
D) \[{{C}_{8}}{{H}_{18}}\]
Correct Answer: C
Solution :
| [c] \[d=\frac{pM}{RT}\] |
| \[M=\frac{dRT}{pM}=\frac{2.28\times 0.081\times 300}{1}=56.20\,\text{g/mol}\] |
| Ratio \[\Rightarrow \] \[\frac{85.7}{12}:\frac{14.3}{1}=1:2\] |
| Empirical formula of compound \[={{(C{{H}_{2}})}_{n}}\] |
| \[n=\frac{56.20}{12+2}=4\] |
| Molecular formula \[=[C{{H}_{2}}]\times 4={{C}_{4}}{{H}_{8}}\] |
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