Enthalpy of combustion of carbon to `CO_(2)` is `-393.5 kJ mol^(-1)`. Calculate the heat released upon formation of `35.2 g` of `CO_(2)` from carbon and dioxygen gas.

Options

A. 214.8 kJ
B. -314.8 kJ
C. 414.8 kJ
D. 514.8 kJ

Answer

B

Explanation

`DeltaH_("combusion")= -393 kJ//mol`
i.e, 1 mole of `CO_(2)` on combustion release= -393
`(35.2)/(44)` moles `CO_(2)` will release = `(13852.2)/(44)= -314.8 kJ`