Chemistry

Chemistry

Problem

At 298 K298\,\text{K} the decomposition reaction 2 NH3(g)  →  N2(g)+3 H2(g)\mathrm{2\,NH_3(g)\;\rightarrow\;N_2(g)+3\,H_2(g)} has ΔSrxn∘=198  J mol−1 K−1\Delta S^{\circ}_{\text{rxn}} = 198\;\text{J\,mol}^{-1}\,\text{K}^{-1}. Given S∘ ⁣(N2(g))=192  J mol−1 K−1S^{\circ}\!(\mathrm{N_2(g)}) = 192\;\text{J\,mol}^{-1}\,\text{K}^{-1} and S∘ ⁣(H2(g))=131  J mol−1 K−1S^{\circ}\!(\mathrm{H_2(g)}) = 131\;\text{J\,mol}^{-1}\,\text{K}^{-1}: (a) Determine S∘ ⁣(NH3(g))S^{\circ}\!(\mathrm{NH_3(g)}) at 298 K298\,\text{K}. (b) The literature value for S∘ ⁣(NH3(g))S^{\circ}\!(\mathrm{NH_3(g)}) is 193  J mol−1 K−1193\;\text{J\,mol}^{-1}\,\text{K}^{-1}. Calculate the percent error of your value relative to the literature value. a. Determine S∘ ⁣(NH3(g))S^{\circ}\!(\mathrm{NH_3(g)}) at 298 K298\,\text{K}. b. Calculate the percent error relative to the literature value given.

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