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exam 3 practice

# exam 3 practice - Resource Page Periodic Table of the...

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Resource Page Periodic Table of the Elements Nernst equation: Q n V E Q n V E Q nF RT E E log 05917 . 0 ln 025693 . 0 ln - ° = - ° = - ° = (at T = 298.15K) Arrhenius equation: ) / exp( RT E A k a - = Reduction half-reaction E° (V) ClO 4 - + 2H + + 2 e - barb2right ClO 3 - + H 2 O +1.23 Ag + + e - barb2right Ag +0.80 Pb 2+ + 2 e - barb2right Pb -0.13 Atomic masses Iodine = 126.90 g/mol Hydrogen = 1.008 g/mol R = 1.3807E-23 J/K N A = 6.022E23 particles/mol

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Chemistry 204 Practice Exam 3 – 40 minutes 1. Balance the following electrochemical equation in acidic condition using the smallest whole-number coefficient. What is the reaction quotient (Q) for the following reaction? Ag(s) | Ag + (aq) || ClO 4 - (aq), H + (aq), ClO 3 - (aq) | Pt (s), E = +0.40 V. 2. A lead electrode (cathode) in 0.010 M Pb(NO 3 ) 2 (aq) is connected to a hydrogen electrode (anode) in which the pressure of H 2 is 0.057 V at 25 °C. What is the pH of the electrolyte at the hydrogen electrode? 3. When 0.52 g of H 2 and 0.19 g of I 2 are confined to a 750-mL reaction vessel and heated to 700 K, they react by a second-order process (first order in each reactant), with k = 0.063 L/(mol*s) in the rate law (for the rate of formation of HI). (a) What is the initial rate? (b) By
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