What is the ∆G for the following reaction under standard conditions (T = 298 K) for the formation of NH4NO3(s)? 2NH3(g) + 2O2(g)
NH4NO3(s) + H2O(l)
Given:
NH4NO3(s): ∆Hf = -365.56 kJ ∆Sf = 151.08 J/K.
NH3(g): ∆Hf = -46.11 kJ ∆Sf = 192.45 J/K.
H2O(l): ∆Hf = -285.830 kJ ∆Sf = 69.91 J/K.
O2(g): ∆Hf = 0.00 kJ ∆Sf = 205 J/K.
1 answer:
∆G = ∆H - T<span>∆S
NH3: </span><span>∆G = -46.11x10^3 - (298)(192.45) = -103460.1 J
O2: </span><span>∆G = 0 - (298)(205) = -61090 J
NH4NO3:</span><span> ∆G = -365.56x10^3 - (298)(151.08) = -410581.84 J
H2O:</span> ∆G = -285.830x10^3 - (298)69.91) = -306663.18 J
∆Grex = ∆Gproducts - ∆Greactants
∆Grex = (-410581.84 + -306663.18) - (-103460.1/2 + -<span>61090/2)</span>
∆Grex =-634969.97 J/mol = -634.97 kJ/mol
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