5. What is the reduction potential for this half cell: AgAg+(105M);EAg+,Ag+=0.80V. (A) 0.80V (B) 1.3V (C) 0.5V (D) 0.50V 6. Calculate Kp for this equilibrium at 450C:H2(g)+I2(g)2Hl(g), when the equilibrium concentrations of H2(g)=0.17M,I2(g)=0.17M, and Hl(g)=3.34M at the same temperature. (A) 1.5105 (B) 9.0108 (C) 2.3106 (D) 386 7. Calculate Gibbs energy (G) at 25C for the reaction: ZnS(s)+1.5O2(g)ZnO(s)+SO2(g). Given that the partial pressures of O2(g)=1.7atm, and SO2(g)=0.15atm, and Gr(ZnS(s))=147kJmol1,Gr(ZnO(s))= 318kJmol1,Gi(SO2(g))=300kJmol1 (A) 478kJmol1 (B) 6491kJmol1 (C) 7135kJmol1 (D) 454kJmol1 8. Calculate the standard Gibbs energy change at 600K for the reaction: N2O4(g)2NO2(g). Given that Gr(N2O4(g))=+97.9kJmol1,Gr(NO2(g))=+51.3kJmol1,H(N2O4(g))=+9.2kJmolmol1, and HP(NO2(g))=+33.3kJmol1 at 298K. (A) 30.8kJ (B) 48.6kJ (C) 67.5kJ (D) +67.5kJ 9. Calculate Ssystm when the state of 1.0mol of gas (Cpm=3.5R), is changed from 25C and 1.50atm to 135C and 7.00atm. (A) 71.4J/K (B)+71.4J/K (C) 35.7J/K (D) 54J/K 10. Calculate the molar entropy of a constant-volume sample of argon at 250K given that it is 154.84J K1mol1 at 298K; the molar constant-volume heat capacity of argon is I.5R. (A) +153Jmol1K1 (B) +165Jmol1K1 (C) 165Jmol1K1 (D) 153Jmol1K1