A) 0.2 N
B) 0.01 N
C) 0.001 N
D) 0.02 N
Correct Answer: B
Solution :
Key Idea According to Faradays first law W = ZIt where, W = mass of substance deposited (gram) I = current (amperes) t = time (second) Z = electrochemical equivalent and \[Z=\frac{E}{96500}\] where, E = equivalent weight \[E=\frac{atomic\text{ }weight}{valency}\] Here, \[I=\,1\,A\], Molar mass of copper = 63.5 t=16 min and 5 s \[=16\times 60+5=965\,s\] Using formula \[m=\frac{E}{96500}\times I\times t\] \[=\frac{63.5/2}{96500}\times 1\times 965\] \[=\frac{63.5}{200}=0.3175\,g\] Volume of \[CuC{{l}_{2}}\] solution = 1 L \[\because \] Normality \[=\frac{weight\text{ }of\text{ }solute/eq.\text{ }wt.\text{ }of\text{ }solute}{volume\text{ }of\text{ }solution\text{ }\left( in\text{ }litre \right)}\] \[\therefore \] Normality of \[CuC{{l}_{2}}\] solution \[=\frac{0.3175}{31.75\times 1}\] = 0.01 N
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