ThermochemistryHard
Question
Determine enthalpy of formation for H2O2 (l), using the listed enthalpies of reactions :
N2H4 (l) + 2H2O2 (l) → N2 (g) + 4H2O (l); ᐃrHo1 = - 818 kJ/mol
N2H4 (l) + O2 (g) → N2 (g) + 2H2O (l); ᐃrHo2 = - 622 kJ/mol
H2 (g) +
O2 (g) → H2O (l); ᐃrHo3 = - 285 kJ/mol
N2H4 (l) + 2H2O2 (l) → N2 (g) + 4H2O (l); ᐃrHo1 = - 818 kJ/mol
N2H4 (l) + O2 (g) → N2 (g) + 2H2O (l); ᐃrHo2 = - 622 kJ/mol
H2 (g) +
O2 (g) → H2O (l); ᐃrHo3 = - 285 kJ/molOptions
A.-383 kJ/mol
B.-187 kJ/mol
C.-498 kJ/mol
D.None of these
Solution
For H2(g) + O2(g) → H2O2(l)
DfHo (H2O2,l) = ᐃrH3o +
DfHo (H2O2,l) = ᐃrH3o +
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