Calculate the emf of the following concentration cell:
Mg(s) | Mg2+(0.15 M) ||
Mg2+(0.82 M) | Mg(s)
V?
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11.) Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reactions at 25 C. Write the equation for the cell reaction that occurs under standard-state conditions. 12.) Calculate the emf and then predict whether the following reaction would occur spontaneously in aqueous solutions at 25 C. Assume that the initial concentrations of dissolved species are all 1.0 M. Show calculations. a.) Care) + Cd2+ (aq) → Ca2+ + Cd() b.) Br2() + Sn(3) ► 2Br...
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Calculate Eº, E, and AG for the following cell reactions (a) Mg(s) + Sn2+(aq) =Mg2+(aq) + Sn(s) where [Mg2+] = 0.040 M and [Sn2+] = 0.045 M 8° = 2.23 10 E = 2.23 AG=430390 (b) 3Zn(s) + 2Cr3+(aq) = 3Zn2+(aq) + 2Cr(s) where [Cr3+] = 0.040 M and [Zn2+] = 0.0065 M E° = 0.03 E = 0.0671 AG=-0.0389
When the Cu concentration is 1.08 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.810V. What is the Mg concentration? Cu2 (aq)Mg(s) »Cu(s) + Mg2 (aq) Answer
When the Cu concentration is 1.08 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.810V. What is the Mg concentration? Cu2 (aq)Mg(s) »Cu(s) + Mg2 (aq) Answer