19 Questions
What is the standard cell potential (Eocell) for the cell formed by the half-reactions Fe3+ + e- → Fe2+ and Zn2+ + 2e- → Zn?
1.53 V
A Pt | H2; p1/solution of H2 ions / Pt | H2; p2 cell represents:
Electrode concentration cell
In the galvanic cell prepared using zinc and iron, what reaction occurs at the cathode?
Fe2+ → Fe3+ + e-
Which of the following factors does not affect the electrode potential of an electrode?
Size of the electrode
If a hydrogen electrode is dipped in a solution of pH 3 at 25°C, what would be the potential?
-0.210 V
If the salt bridge is removed between two half-cells, what happens to the voltage?
Decrease to be zero
What is the closeness of the experimental results, or mean of a number of results, to the true value called?
Accuracy
In a galvanic cell using zinc and iron, what reaction occurs at the anode?
Zn → Zn2+ + 2 e-
An electrolyte is a substance which:
when dissolved in water, dissociates into ions
What defines strong electrolytes?
dissociate into ions even at high concentration
Why does an electrochemical cell stop working after some time?
one of the electrodes is eaten away
Which statement is not true for a standard hydrogen electrode?
It contains a metallic conductor which does not absorb hydrogen
What defines a half-cell reaction?
takes place at one electrode
What are the advantages of electrochemical analysis due to?
all the above
What does the standard hydrogen electrode consist of?
Platinum black foil (Platinum inert electrode)
The significant disadvantage of the saturated calomel electrode (SCE) is
its potential is sensitive to changes in temperature
The reference electrode that is thermally more stable is:
Ag/AgCl electrode
In an electrolytic cell, which of the following is the half-cell where reduction takes place.
Cathode
Mercury covered by a layer of mercurous chloride in contact with saturated potassium chloride solution is a description of which electrode?
Reference electrode
Test your knowledge of galvanic cells in electroanalytical chemistry with these questions about cell notation and half-reactions. Determine the reactions at the cathode and calculate the Eocell for specific half-reactions.
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