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
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Thermochemical Equation concept. You can view video lessons to learn Thermochemical Equation. Or if you need more Thermochemical Equation practice, you can also practice Thermochemical Equation practice problems.