What is using these equations below calculate the enthalpy for the reaction : 2H2 (g) + O2 (g) -> 2H2O (g) ΔH = ? 1. 2O (g) -> O2 (g) ΔH= -294 kj/mol 2. H2O (l) -> H2O (g) ΔH= 44 kj/mol 3. 2H (g) + O (g) -> H2O (g) ΔH= -803 kj/mol 4. C (gr.) + 2O (g) -> CO2 (g) ΔH= -643 kj/mol 5. C (gr.) + O2(g) -> CO2 (g) ΔH= -394 kj/mol 6. C (gr.) + 2H2 (g) -> CH4 (g) ΔH= -75 kj/mol 7. 2H (g) -> H2 (g) ΔH= -436 kj/mol 8. H20 (l) -> H20 (g) ΔH= 10.25 kj/mol (gr.) stands for graphite. I am wondering if you can multiply an equation by the value zero because there is no CH4 (g) in the final equation ?
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jerichorayel
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Can you try to check the values? I see the items 2 and 8 have the same equation but have different delta H values. Another thing, if we try to add the combustion of methane (CH4), we can probably solve the problem.
CH4(g) + 2O2 (g) --->2 H2O (g) + CO2 (g) delta H = -891 kJ/mol
If ever the equation I mentioned will be included, we can find the reaction using Hess's law.
4O (g) --> 2O2 (g) ΔH x 2
4H2O (l) --> 4H2O (g) ΔH x 4
2H2O (g) --> 4H(g) + 2O (g) ΔH x(-2)
4H (g) --> 2H2 (g) ΔH x 2
CO2(g) --> C(gr) + 2O(g) ΔH x (-1)
CO2(g) --> C(gr) + O2(g) ΔH x (-1)
2C(gr) + 4H2(g) --> 2CH4 (g) ΔH x 2
2CH4(g) + 4O2 (g) --> 4H2O(l) ΔH x 2
+2CO2(g)
-----------------------------------------------
2H2 + O2 ---> 2H2O
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