Use cell potential to calculate an equilibrium constant. Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: Cu2+(aq) + Fe2+(aq) Cu+(aq) + Fe3+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: Use measured cell potential to calculate concentration. When [Ag] 1.18 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 3.283 V. What is the Mg2+ concentration in this cell? 2Ag (aq) + Mg(s) 2Ag(s) + Mg2+(aq) [Mg2+]= M

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Use cell potential to calculate an equilibrium constant.
Calculate the cell potential and the equilibrium constant for the following reaction at 298 K:
Cu2+(aq) + Fe2+(aq) Cu+(aq) + Fe3+(aq)
Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the
antilogarithm.
Equilibrium constant:
Transcribed Image Text:Use cell potential to calculate an equilibrium constant. Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: Cu2+(aq) + Fe2+(aq) Cu+(aq) + Fe3+(aq) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant:
Use measured cell potential to calculate concentration.
When [Ag] 1.18 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 3.283
V. What is the Mg2+ concentration in this cell?
2Ag (aq) + Mg(s) 2Ag(s) + Mg2+(aq)
[Mg2+]=
M
Transcribed Image Text:Use measured cell potential to calculate concentration. When [Ag] 1.18 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 3.283 V. What is the Mg2+ concentration in this cell? 2Ag (aq) + Mg(s) 2Ag(s) + Mg2+(aq) [Mg2+]= M
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