Copper is to be electrodeposited on a nickel block of (20 5) cm ^2 area by using CuSO ₄ as electrolyte. How much quantity of electricity is needed to deposit a 3.6 m layer of copper? [Atomic weight of Cu =63.5 ~mol ⁻¹ Density of . CuSO ₄=8.9 ~g / cc ]

Step-by-step solution

W= E Q F = A n Q F aligned A^ & h d= A Q n F Q & = (A^ h ) d n F A & = 0.036 8.9 2 96500 63.5 =973.814 C 974 C aligned [ Volume of Cu-deposited on the nickel block = area of the block thickness of copper layer =A^ h=(20 5) (3.6 10⁻⁶ 10^2 ) cm ^3=0.036 ~cm ^3 [ 1 m =10⁻⁶ ~m =10⁻² 10^2 ~cm ] Where, d= density of Cu =8.9 ~g / cm ^3 aligned & n=2 & F=96500 C mol ⁻¹ & A= atomic weight of Cu ^*=63.5 ~g ~mol ⁻¹ & lata informations, & density of CuSO . Cu ₄²⁺+2 e⁻ Cu ] & rong : it will be density of Cu =8.9 ~g / cc ] align