A) 35.77 kJ
B) 98.38 kJ
C) 1574.08 kJ
D) 393.52 kJ
Correct Answer: B
Solution :
The heat released upon formation of \[\text{C}{{\text{O}}_{\text{2}}}\]will be \[\text{+}\,\,\text{393}\text{.52 kJ/mol}\] 1 mol \[C{{O}_{2}}=44\,g\]of \[\text{C}{{\text{O}}_{\text{2}}}\] So, for 44 gm of\[\text{C}{{\text{O}}_{\text{2}}}\]formation energy released is \[\text{+}\,\text{393}\text{.52 kJ}\] \[\therefore \] for 11 g of \[\text{C}{{\text{O}}_{\text{2}}}\] formation energy released \[=\frac{393.52}{44}\times 11\] \[=98.38\,kJ\]
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