A) \[\text{110}\text{.5kJ}\]
B) \[\text{676}\text{.5 kJ}\]
C) \[-\text{676}\text{.5 kJ}\]
D) \[-\text{110}\text{.5kJ}\]
Correct Answer: A
Solution :
(i) \[C(s)+{{O}_{2}}(g)\xrightarrow{{}}C{{O}_{2}}(g);\] \[\Delta H=-393.5\,kJ\] (ii) \[CO(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}C{{O}_{2}}(g);\] \[\Delta H=-283.0\,kJ\] On subtracting Eq. (II) from Eq. (I), we get (iii) \[C(s)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}CO(g);\] \[\Delta \Eta =-110.5\,kJ\] The equation III also represents formation of 1 mole of CO and thus, enthalpy change, ie, \[-110.5\,kJ,\]is the heat of formation of \[CO(g).\]You need to login to perform this action.
You will be redirected in
3 sec