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1. Calculate the standard entropy change for the following reaction, 2 HgO(s) 2 Hg(l) + O2(g) given s°[ggO] = 70.3 J/K-mol, 5°I Hg(1)] =76.0 J/K.mol, and 5°[O2(g)] = 205.1 J/K.mol. 2. For a reaction, AH = +62.9 kJ and AS = +132.9 J/K. At what temperature will AG =0.00kJ? 3. The standard free energy change for the formation of N2H4(l) from elements is +149 kJ/mol at 25 °C. What is the equilibrium constant for the reaction? (R = 8.314 J/K.mol) 4. Calculate E for the following electrochemical cell at 25 °C Pt(s) | Sn2*(aq, 0.50 M), 0.50 M) Il T(aq, 0.15 M) | Agl(s) | Ag(s) given the following standard reduction potentials. Agl(s) + e Ag(s) + T(aq) E° = -0.15 V Sn4' (aq) + 2 e Sn2t(aq) = +0.15 V 5. If AG for the following reaction is -324 kJ, calculate Cr2O7 (aq) + 2 Fe(s) + 14 H^(aq) (aq) + + 7H2O(l)

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