Standard enthalpies of formation

Question

Assignment:

Use some or all of the following reaction enthalpies to calculate delta H for the reaction:

3NH₃(aq) + ClO- (aq) --> N2H4(g) + NH4+ (aq) + Cl- (aq) + OH- (aq)

Cl^- (aq) + H₂O₂(l) --> H₂O(l) + ClO- (aq) delta H = - 6.5kJ/mol
N₂(g) + 3H₂(g)--> 2NH₃(g) delta H = -160.6kJ/mol
H₂O(l) + 1/2 N2H4(g) --> 1/2 H₂O₂(l) + NH3(aq) delta H = + 63.9kJ/mol
3H₂(g) + 2 ClO₂^- (aq) --> ClO^- (aq) + Cl^- (aq) + 3H₂O(l) delta H = - 424.9 kJ/mol
NH₃ (aq) + H₂O (l) --> NH₄⁺ (aq) + OH- (aq) delta H = + 3.6 kJ/mol

Use the standard enthalpies of formation to calculate delta H for the reaction of ammonia and hypochlorite shown above: delta H formation (NH₃(aq)) = - 80.3 kJ/mol; delta H formation (ClO^-(aq) = -75.7 kJ/mol; delta H formation (N₂H₄(g)) = +95.4 kJ/mol; delta H formation (NH₄⁺(aq)) = - 132.5 kJ/mol; delta H formation (Cl^-(aq) = - 167.2 kJ/mol; delta H formation (OH-(aq)) = -230.0 kJ/mol

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