Given the following thermochemistry equations: NH4NO2(s) -------> N2 (g) + 2H2O(l); ΔH = -300.12 kJ/mol NH3...

Given the following thermochemistry equations:

NH4NO2(s) -------> N2 (g) + 2H2O(l); ΔH = -300.12 kJ/mol

NH3 (aq) + HNO2 (ac) ------> NH4O2 (aq); ΔH = -38.04 kJ/mol

NH402(s) -------> NH402(aq); ΔH = 19.85 kJ/mol

H2 (g) + 1/2 O2 (g) ------> H2O (l) ΔH = -284.24 kJ/mol

1/2 N2 (g) + 3/2 H2 (g) ------> NH3(ac) ΔH = -85.27 kJ/mol

Calculate the ΔH for the formation of HNO2

Expert Solution

queen_honey_blossom answered 2 years ago

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