Calculate delta H for C+ 1/2 O2 --> CO
given:
C+ O2, delta H = -22kj
CO + 1/2 O2 --> Co2, delta H = -15kj
Our target equation is
C(s) + (1/2)O2(g) → CO(g); ΔH=?
We have the following information:
1. C(s) + O2(g) →
CO2(g); ΔH= -22 kJ
2. 2CO(g) + O2 → 2CO2(g); ΔH= -15
kJ
To solve this problem, we use Hess's Law.
Our target equation has C(s) on the left hand side, so we re-write equation 1:
1. C(s) + O2(g) → CO2(g); ΔH= -22 kJ
Our target equation has CO(g) on the right hand side, so we reverse
equation 2. (2CO(g) + O2 → 2CO2(g); ΔH= -15 kJ) and divide by 2.
3. CO2(g) → CO(g) + (1/2)O2; ΔH=+7.5 kJ
It will the change the sign of ΔH and value as it also divide by 2 as shown above
Then we add equations 1 and 3 and their ΔH values.
This gives
C(s) +(1/2)O2(g) → CO(g); ΔH=-14.5 kJ
Using your numbers, the
standard enthalpy of formation of carbon monoxide is
-14.5 kJ/mol.
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