We’re being asked to determine the enthalpy change when 2.66 g H2O is produced.
The given reaction is:
H2(g) + 1/2 O2(g) → H2O(g); ΔH = –286 kJ/mol
From the balanced equation, we can see that the given ΔH˚rxn (-286 kJ/mol) corresponds to 1 mole of H2O.
For the reaction
H2(g) + 1/2O2(g) --> H2O(l) deltaH = –286 kJ/mol
calculate the enthalpy change when 2.66 g of water is produced.
1. 761 kJ
2. –42.2 kJ
3. –761 kJ
4. 108 kJ
5. 42.2 kJ
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