Given that: C(s) + (g) - (g); δ H° = -X kJ and 2(g) + (g) - 2(g); δ H° = -Y kJ. The enthalpy of formation of carbon monoxide will be

Question

Given that: C(s) + $O_2$(g) -> $CO_2$(g); δ H° = -X kJ and 2$CO$(g) + $O_2$(g) -> 2$CO_2$(g); δ H° = -Y kJ. The enthalpy of formation of carbon monoxide will be

Prashant Kotian · Accepted Answer

Correct answer: B. We want the formation of : C(s) + 1/2 (g) -> (g). Let's use the given reactions: (1) C(s) + (g) -> (g); δ H1 = -X. (2) (g) + 1/2 (g) -> (g); δ = -Y/2 (by dividing the second given equation by 2). Subtracting (2) from (1): C(s) + 1/2 (g) -> (g); δ H = δ H1 - δ = -X - (-Y/2) = (Y - 2X)/2.

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