MCQ
In the reaction,


- ✓$ \mathrm{C}_6 \mathrm{H}_5 \mathrm{SO}_3 \mathrm{H} $
- B$ \mathrm{C}_6 \mathrm{H}_5 \mathrm{OH} $
- C$ \mathrm{C}_6 \mathrm{H}_5 \mathrm{SO}_2 $
- D$ \mathrm{C}_6 \mathrm{H}_5 \mathrm{CHO}$

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${H_2} + \frac{1}{2}{O_2} \to \,{H_2}O + 68.3\,kcal$
$C{H_4} + 2{O_2}\, \to \,C{O_2} + 2{H_2}O + 210.8\,kcal$ Then the possible heat of methane will be.....$ kcal$
$C{H_4}(g) + 2{O_2}(g) \to C{O_2}(g) + 2{H_2}O(l)$ ;
${\Delta _r}{H_{300}} = - 212.7\ Kcal / mol$ .
The absolute value of ${\Delta _r}U_{300}^o$ for this reaction is .......$Kcal\,/\,mol$ $(R = 2\ cal/mol-K)$