MCQ
During complete combustion of one mole of butane, $2658kJ$ of heat is released. The thermochemical reaction for above change is :
- A$2\text{C}_4\text{H}_{10}(\text{g})+130_2(\text{g})\rightarrow $$ 8\text{CO}_2({\text{g})}+10\text{H}_2\text{O}(\text{l})\Delta_\text{c}\text{H}=-2658.0\text{kJ}\ \text{mol}^{-1}$
- B$\text{C}_4\text{H}_{10}(\text{g})+\frac{13}{2}\text{O}_2(\text{g})\rightarrow $$ 4\text{CO}_2(\text{g})+5\text{H}_2\text{O}(\text{g})\Delta_\text{c}\text{H}=-1329.0\text{kJ}\ \text{mol}^{-1}$
- ✓$\text{C}_4\text{H}_{10}+\frac{13}{2}\text{O}_2(\text{g})\rightarrow4 $$ \text{CO}_2(\text{g})+5\text{H}_2\text{O}\text{}(\text{l})\Delta_\text{c}\text{H}=-2658.0\text{kJ}\ \text{mol}^{-1}$
- D$\text{C}_4\text{H}_{10}(\text{g})\frac{13}{2}\text{O}_2(\text{g})\rightarrow $$ 4\text{CO}_2(\text{g})+5\text{H}_2\text{O}(\text{l})\Delta_\text{c}=+2658.0\text{kJ}\ \text{mol}^{-1}$