A. Calculate ΔG° and log Kc for the following reaction at 298 K:
Given: 
B. Using the 
values of A and B, predict which is better for coating the surface of iron to prevent corrosion and give reasons.
,
OR
A. The conductivity of 0.001 mol L-1 solution of CH3COOH is 3.905× 10-5 S cm-1. Calculate its molar conductivity and degree of dissociation (α).
Given: 
and
B. What type of battery is dry cell? Write the overall reaction occurring in dry cell.
A.
For a chemical reaction,
n = number of electrons transferred
For the reaction,
Also we know that for a electrolytic cell,
Ans
ΔG° = 1169.58 kJ log KC = 0.47206
B.
Prevention of corrosion is done by coating a material by more reactive metal than iron, so that iron does not rust or react in presence of moisture. The given are the reduction potential of metals. Thus the one with lowest reduction potential will oxidize faster as compared to iron i.e. the one with highest reduction potential should be coated.
As E° of B is less than both Fe and metal A it will undergo reduction faster as compared to iron and would not prevent corrosion.
Mathematically,
As 
metal A is preferred as a coating material.
OR
A.
Given: conductivity (k) = 3.905×10-5 S cm-1
Concentration (c) = 0.001 × 10-3 mol cm-3
Formula: 
Solution:
Also for a electrolyte,
Molar conductivity is 
Degree of dissociation = 39.05/390.5 = 0.1
B.
Dry cell consists of a zinc metal casing which acts as the anode and a carbon (graphite rod) which acts as cathode. The electrochemical reaction between the zinc and carbon generates electric potential. A typical dry cell provides 1.5 V of direct current. The two electrodes are separated by a paste of ammonium chloride which acts as an electrolyte.
Chemical reactions involved in a dry cell are:
Anode reaction:
Cathode reaction:
Overall general reaction:
Couldn't generate an explanation.
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