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WorksheetsElectrochemical Cells Quiz
Total questions: 10
Worksheet time: 9mins
What is a galvanic cell and how does it work?
A galvanic cell is a device that converts mechanical energy into electrical energy.
A galvanic cell is a type of fuel cell that uses hydrogen as the fuel to generate electricity.
A galvanic cell is an electrochemical cell that generates electrical energy from non-spontaneous chemical reactions.
A galvanic cell is an electrochemical cell that generates electrical energy from spontaneous chemical reactions.
What are the differences between galvanic cells and electrolytic cells?
Galvanic cells convert electrical energy into chemical energy, while electrolytic cells convert chemical energy into electrical energy.
Galvanic cells convert chemical energy into electrical energy, while electrolytic cells use electrical energy to drive a non-spontaneous chemical reaction.
Galvanic cells use electrical energy to drive a non-spontaneous chemical reaction, while electrolytic cells convert chemical energy into electrical energy.
Galvanic cells and electrolytic cells both convert chemical energy into electrical energy.
Calculate the cell potential for a galvanic cell with a standard electrode potential of E cathode=+0.80V and E anode-0.60V.[Given values are reduction Potentials]
-0.20V
2.40V
0.20V
1.40V
What is the standard electrode potential for cathode of a galvanic cell with a cell potential of 1.23V and an EM|M+ 0.80V?
0.43V
2.03V
0.63V
1.03V
Metal(X) | salt (X)| ions(X) || ions(Y) | salt(Y) | Metal(Y)
X=LHS Y=RHS
X=Cathode
Y=Anode
X=Anode
Y=Cathode
X=Cathode
Y=Anode
X=Anode
Y=Anode
The correct match among the following is:
Cathode=Reduction
Anode=Reduction
Cathode=Reduction
Anode=Oxidation
Cathode=Oxidation
Anode=Oxidation
Cathode=Oxidation
Anode=Reduction
Cr2+ + 2e- ------->Cr
The above reaction is an example of_________reaction which takes place at ____________.
Reduction, Anode
Reduction,Cathode
Oxidation, Anode
Oxidation, Cathode
The Standard Cell potential of an electrochemical cell (in V)
Cu|Cu2+||Ag+|Ag
Given: E0 Cu2+|Cu=0.337V and E0 Ag+|Ag=0.80V
(a)
For the reaction to be spontaneous Change in Gibbs Free Energy(G) and Ecell should be ______ & __________ respectively
Positive and Negative
Negative and positive
Negtive and negative
Positive and positive
Pt,H2(1atm) | HCl (1.0M)
For the above cell at 298K E0 = (a) V
