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Problem: For the reactionH2(g) + 1/2O2(g) --> H2O(l)              deltaH = –286 kJ/molcalculate the enthalpy change when 2.66 g of water is produced.1. 761 kJ2. –42.2 kJ3. –761 kJ4. 108 kJ5. 42.2 kJ

FREE Expert Solution

We’re being asked to determine the enthalpy change when 2.66 g H2O is produced

The given reaction is:

2(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

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Problem Details

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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