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WorksheetsElectrochemistry
Total questions: 15
Worksheet time: 12mins
Given their standard reduction potentials, which of the species is going to be oxidized?
Cu2+/Cu = 0.34V
Zn2+/Zn = -0.76V
Cu
Zn
CuSO4
ZnSO4
What reaction occurs at the anode?
Ag+/Ag = 0.80V
Ni2+/Ni = -0.25V
Ag+ + e- →Ag
Ag → Ag+ + e-
Ni2+ + 2e- → Ni
Ni → Ni2+ + 2e-
What is a reducing agent?
It is the species that gets reduced -- gains electrons.
It is the species that gets oxidized -- loses electrons.
It is the species that creates electrons.
It is the species that destroys electrons.
In the following reaction
Sn+2 + 2Fe+3 → Sn+4 + 2Fe+2
the oxidizing agent is....
Sn+4
Sn+2
Fe+3
Fe+2
When water is electrolyzed, gas collected at cathode, is
sulphur
oxygen
hydrogen
sulphur dioxide
Galvanic cells convert
mechanical energy in to electrical energy
potential energy in to electrical energy
electrical energy in to chemical energy
chemical energy in to electrical energy
Consider this cell.
Select all true statements
Zinc is a more reactive metal than copper
Cu2+ is a stronger oxidising agent that Zn2+
The cell potential is the sum of the two electrode potentials
The copper electrode will get bigger as current flows
The zinc electrode will get smaller as current flows
Rusting is a special term, given to the corrosion metal is... .
Au
Pt
Fe
Ag
What two things cause Iron to Rust ?
Air and Oxygen
Oxygen and Water
Water and Carbon dioxide
Carbon dioxide and Air
Which diagram shows the most favourable conditions for rust to appear on the nail?
A
B
C
D
Rusting can be prevented by
Alloying
Tinning
Galvanizing
All of above
Observe the picture...and select the appropriate options
Forward reaction= Extraction of metals from ore
Backward reaction= Corrosion
Corrosion phenomenon will be Spontaneous
Metals are more stable in the Ore form (naturally occurring form)
Name any way of preventing corrosion other than Galvanizing, tinning & alloying. (very commonly applied method at every home)
