A) \[110.5kJ\]
B) \[676.5\text{ }kJ\]
C) \[-\text{ }676.5\text{ }kJ\]
D) \[-110.5kJ\]
Correct Answer: D
Solution :
I: \[C(s)+{{O}_{2}}(g)\xrightarrow{{}}C{{O}_{2}}(g);\]\[\Delta H=-393.5kJ\] II:\[CO(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}CO(g);\]\[\Delta H=-283.0kJ\] Substracting (I) from (II) III:\[C(s)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}CO(g),\]\[\Delta H=-110.5kJ\] This equation (III) also represents formation of one mole of CO and thus enthalpy change is the heat of formation of\[CO(g)\].
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