UNIT 2: Electrochemistry

Electrochemical corrosion involves:

Corrosion increases with:

Fuel cell example:

Sacrificial protection uses:

Galvanization prevents corrosion by:

Rusting of iron requires:

Corrosion is:

Fuel cells convert:

Dry cell is:

Lead accumulator is a:

Equivalent conductivity increases with:

Conductivity decreases with dilution for:

Electrolysis requires:

During electrolysis, reduction occurs at:

1 Faraday =

Faraday’s law relates:

Unit of resistivity:

Kohlrausch’s law applies to:

Molar conductivity increases with dilution because:

Specific conductance is:

K (equilibrium constant) increases with:

If E°cell is negative:

Larger E°cell means:

E°cell = E°cathode – E°anode

Increase in temperature generally:

When ΔG = 0, reaction is:

F (Faraday constant) equals:

Value of n in equation refers to:

At higher concentration, EMF generally:

Nernst equation includes factor:

Relation between ΔG° and E° is:

Standard hydrogen electrode potential is:

ΔG = –nFE, if E is positive then ΔG is:

At equilibrium, EMF is:

Nernst equation relates EMF with:

Unit of molar conductivity:

Weak electrolytes:

Strong electrolytes show:

Electrochemical series is based on:

Cathode in galvanic cell is:

Oxidation is:

Conductivity depends on:

The SI unit of conductance is:

In electrolytic cells, anode is:

The function of salt bridge is:

EMF of Daniell cell is approximately:

Reduction occurs at:

Standard electrode potential is measured at:

The unit of EMF is:

In a galvanic cell, oxidation occurs at: