A) The reaction of 0.624 mole of Al
B) The formation of 0.624 mole of \[A{{l}_{2}}{{O}_{3}}\]
C) The reaction of 0.312 mole of Al
D) The formation of 0.150 mole of \[A{{l}_{2}}{{O}_{3}}\]
Correct Answer: B
Solution :
| [b] \[2\,Al+\frac{3}{2}{{O}_{2}}\xrightarrow{{}}A{{l}_{2}}{{O}_{3}};\] |
| \[\Delta {{H}^{o}}=-\,837.8\,kJ\,mo{{l}^{-1}}\] |
| 2 mol 1.5 mol 1 mol |
| 1 mol 0.75 mol 0.5 mol |
| \[837.8\,kJ\,mo{{l}^{-1}}\equiv \]Combustion of 1 mole Al or formation of 0.5 mole \[A{{l}_{2}}{{O}_{3}}\] |
| \[250\,kcal=\frac{250\times 8.314}{2}\,kJ\] |
| \[=1.24\,mol\,Al\] |
| or \[=0.62\,mol\] of \[A{{l}_{2}}{{O}_{3}}\] |
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