WorksheetsElectrochemistry Quiz
Total questions: 20
Worksheet time: 10mins
Oxidation (modern definition) means:
Gain of electrons
Loss of electrons
Gain of oxygen
Loss of protons
Reduction (modern definition) means:
Loss of electrons
Gain of electrons
Gain of oxygen
Loss of protons
Oxidation and reduction reactions:
Occur separately
Never occur together
Always occur together
Occur only in solutions
In a galvanic cell, oxidation occurs at the:
Cathode
Salt bridge
Anode
Wire
In a galvanic cell, reduction occurs at the:
Anode
Cathode
Salt bridge
External circuit
Electrons flow in a voltaic cell from:
Cathode to anode
Salt bridge to electrode
Anode to cathode
Solution to solution
A galvanic (voltaic) cell reaction is:
Non-spontaneous
Forced by electricity
Spontaneous
At equilibrium
The salt bridge function is to:
Transfer electrons
Maintain electrical neutrality
Increase voltage
Stop ion movement
Cations in a galvanic cell move toward the:
Anode
Cathode
Salt bridge
Wire
Anions in a galvanic cell move toward the:
Cathode
Salt bridge
Anode
Wire
Standard cell potential (E°cell) is measured at:
Any conditions
0°C
25°C, 1 M, 1 atm
High pressure
E°cell is calculated by:
E°anode − E°cathode
E°cathode − E°anode
Sum of half-cell potentials
Product of potentials
If E°cell is positive, the reaction is:
Non-spontaneous
Impossible
At equilibrium
Spontaneous
The standard hydrogen electrode (SHE) has E° equal to:
+1.00 V
−1.00 V
0.00 V
+0.76 V
All standard reduction potentials are measured relative to:
Zn electrode
Cu electrode
Ag electrode
SHE
The more positive the reduction potential, the stronger the:
Reducing agent
Oxidizing agent
Acid
Base
The most negative E° corresponds to the strongest:
Oxidizing agent
Reducing agent
Catalyst
Acid
Reversing a half-reaction causes E° to:
Stay the same
Become zero
Change sign
Double
At equilibrium, the cell potential (E) is:
Maximum
Negative
Zero
Infinite
The Nernst equation relates cell potential to:
Pressure only
Temperature only
Concentration and temperature
Volume only
