Page 1 of 8HOUR EXAM 1 NAME (Print clearly)______________________________ Chemistry 030.102 Last name, first name middle initial Section 1 – Prof. Dagdigian February 24, 2012 jhed ID__________________ Calculators allowed, but do not use programmable features One sheet of paper with notes may be brought into the exam. Miscellaneous information: R= 8.31 J mol–1K–11 J = 1 V-C Faraday's constant F= 96485 C mol–1ΔG°= –nFΔE°ΔE= ΔE°– (RT/nF) lnQ= ΔE°– (0.0592 V/n) logQat 25 °C 1 A = 1 C/sec ΔE°= (RT/nF) lnK= (0.0592 V/n) logKT(K) = T(C) + 273 c= c0e–kt1/c= 1/c0+ 2kt k= Ae–Ea/RTpH = –log[H3O+] 1. Galvanic cells The following standard reduction potentials are available: Ag+(aq) + e–→Ag(s) E°= +0.800 V Co2+(aq) + 2 e–→Co(s) E°= –0.356 V (a) Consider an electrochemical cell containing a cobalt anode immersed a solution Co(NO3)and a silver (Ag) cathode immersed in a solution containing AgNO3. Compute the standard potential difference for this cell. 2
(b) How many minutes will it take to plate 2.5 g of silver on the cathode if the current flowing through the cell were 2.05 A?