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WorksheetsElectrochemistry Basics
Total questions: 10
Worksheet time: 5mins
What is electrode potential?
Electrode potential is the measure of the amount of water in an electrolyte
Electrode potential is the measure of the color change in an electrolyte
Electrode potential is the measure of the temperature of an electrolyte
Electrode potential is the measure of the tendency of an electrode to lose or gain electrons when it is in contact with an electrolyte.
Define standard electrode potential.
Standard electrode potential is the measure of the tendency of a half-cell to form covalent bonds.
Standard electrode potential is the measure of the tendency of a half-cell to gain electrons and be oxidized.
Standard electrode potential is the measure of the tendency of a half-cell to attract protons.
Standard electrode potential is the measure of the tendency of a half-cell to lose electrons and be reduced.
State the Nernst equation.
Ecell = E°cell - (RT/nF) * ln(Q)
Ecell = E°cell + (RT/nF) * ln(Q)
Ecell = E°cell - (RT/nF) * log(Q)
Ecell = E°cell - (RT/nF) * ln(K)
How is cell potential calculated?
Ecell = Ecathode + Eanode
Ecell = Ecathode x Eanode
Ecell = Ecathode / Eanode
Ecell = Ecathode - Eanode
What is the unit of electrode potential?
newtons (N)
joules (J)
volts (V)
amperes (A)
Explain the significance of standard hydrogen electrode.
The significance of the standard hydrogen electrode lies in its role as a reference point for measuring electrode potentials.
The standard hydrogen electrode is primarily used in organic chemistry experiments.
It is a tool for measuring temperature in chemical reactions.
The standard hydrogen electrode is used for electrolysis in batteries.
How does temperature affect the Nernst equation?
Temperature affects the Nernst equation by changing the number of electrons transferred
Temperature affects the Nernst equation by modifying the electrode potential
Temperature affects the Nernst equation by altering the concentration of reactants
Temperature affects the Nernst equation by changing the value of the gas constant (R) and the Faraday constant (F).
Calculate the cell potential when E°cell = 1.23 V and Q = 0.001.
1.230 V
1.220 V
1.234 V
1.4076 V
Determine the standard electrode potential for the reaction Zn(s) + Cu2+(aq) -> Zn2+(aq) + Cu(s).
+0.34 V
-0.76 V
+1.44 V
-1.98 V
If the concentration of Cu2+ ions is 0.1 M and Cu(s) is at 1 atm, calculate the cell potential for the given reaction.
0.25 V
0.42 V
0.18 V
0.34 V
