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You make a cell with a copper electrode in a solution of copper nitrate and a s…

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Wize University Chemistry Textbook > Electrochemistry

Important Equations + Nonstandard conditions (Nernst Equation)

6 Activities

You make a cell with a copper electrode in a solution of copper nitrate and a silver electrode in a solution of silver nitrate.
Cu(s)+2Ag+(aq)⇌Cu2+(aq)+2Ag(s)      E=0.46VCu(s)+2Ag^+(aq)⇌Cu^{2+}(aq)+2Ag(s)\ \ \ \ \ \ E = 0.46 V
If you could increase the concentration of Ag+ , which of the following would be true about the cell potential?

More Important Equations + Nonstandard conditions (Nernst Equation) Questions:
A comproportionation reaction is a reaction where one element in two different oxidation states reacts to form a product where both atoms now have the same oxidation state. An electrochemical cell can be constructed using the comproportionation of cobalt as shown below.
CO3++CO+→2CO2+CO^{3+}+CO^+ \to 2CO^{2+}
If the equilibrium constant for the above reaction is found to be 6.3 x 104 determine the standard cell potential ε0 and draw the electrochemical cell in standard notation
The E° for the reaction of Cu/Cu2+ and Sn/Sn2+ is + 0.19 V. What is the value of the equilibrium constant K for this reaction at 298 K?
Calculate the standard voltage and write the standard cell notation for a galvanic cell composed of the following two half reactions.
Fe2+ + 2e- --> Fe(s) Eo=-0.41V
Cr2O72- + 14H+ + 6e- → 2Cr3+ + 7H2O Eo=1.33V
Electrochemistry: Galvanic cells
For each galvanic cell, what is the value of the equilibrium constant for the reaction between each pair at 25 °C? Please ensure that your answer is specified to two decimal places and that your answer is formatted as follows: 9.15x1025 for both answers.
Ni(s) and Ag+(aq)
Fe(s) and Cr3+(aq)
If you could increase the concentration of Cu2+, which of the following would be true about the cell potential?
Electrochemistry Additional Practice
At 25C, what is the potential of the following cell and what is the Keq?
Ni|Ni2+(aq)(0.010 M)||Cr-(0.20 M)|Cr2(g) | Pt
1) Is the reaction occuring in standard or non-standard conditions?
Gibbs Free Energy and Voltage Practice Problem #1
What is the equilibrium constant for the reaction of copper metal with bromine to form copper(II) ions and bromide ions in aqueous solution at 25oC?
Cu(aq)2++2e−→Cu(s)Eo=+0.34 VBr2(aq)+2e−→2 Br(aq)−Eo=+1.07 V\begin{array}{cc} Cu^{2+}_{(aq)}+2e^- \rightarrow Cu_{(s)} & E^o=+0.34\ V\\ Br_{2(aq)}+2e^- \rightarrow 2\ Br^-_{(aq)} & E^o=+1.07\ V \end{array}