Question

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You have created a galvanic cell in order to perform the following UNBALANCED reaction. First, balance the reaction. Br- + Ag+ → Br2 + Ag

Part 1: You look up the appropriate reduction potentials for this reaction, and you find the following: Half Reaction Eo (V) Br2 + 2e- → 2Br- 1.11 Ag+ + e- → Ag 0.77 What is the voltage of the reaction given in the introduction? Br- + Ag+ → Br2 + Ag

Part 2: We will use this voltage to calculate K and ΔGo. From your balanced reaction, what number will you use for n?

Part 3: In order to calculate K from ΔG, we must select the appropriate value of R. The question, then, is what units will ΔGo have after the calculation. Note that Faraday's constant (F) has a value of 96500 C/mol, E has units of V, n has units of moles, and 1 V = 1 J/C. Which of the following is the correct value for R? A 0.00831 kJ/(mol*K) B 0.0821 L*atm/(mol*K) C 8.31 J/(mol*K)

Part 4: What is the value of ΔGo for the reaction determined in part 1 (in J/mol)?

Part 5: If the above reaction is carried out at 298 K, what is the value of K?

Answer 1