A direct current deposits 54 g of silver (atomic mass =108 ) during the electrolysis. The same quantity of electricity would deposit aluminium (atomic mass =27 ) from aluminium chloride in molten state equal to

Question

A direct current deposits 54 g of silver (atomic mass =108 ) during the electrolysis. The same quantity of electricity would deposit aluminium (atomic mass =27 ) from aluminium chloride in molten state equal to (A) 4.5 g (B) 5.4 g (C) 54 g (D) 27 g

Tardigrade Admin · Accepted Answer

(w1/w2)=(E1/E2) ⇒ (54/w2)=((108/1)/(27)3) E1=(M/n text -factor )=(108/1) for Ag +, E2=(27/3) for Al 3+ ∴ w2=(54 × 9/108)=4.5 g

Q. A direct current deposits $54 g$ of silver (atomic mass $= 108$ ) during the electrolysis. The same quantity of electricity would deposit aluminium (atomic mass $= 27$ ) from aluminium chloride in molten state equal to

4.5 g

5.4 g

54 g

27 g

$\frac{w _{1}}{w _{2}} = \frac{E _{1}}{E _{2}} \Rightarrow \frac{54}{w _{2}} = \frac{\frac{108}{1}}{\frac{27}{3}}$
$∴ w_{2} = \frac{54 \times 9}{108} = 4.5 g$
$E_{1} = \frac{M}{n -factor} = \frac{108}{1}$ for $A g^{+}, E_{2} = \frac{27}{3}$ for $A l^{3 +}$

Q. A direct current deposits 54g of silver (atomic mass =108 ) during the electrolysis. The same quantity of electricity would deposit aluminium (atomic mass =27 ) from aluminium chloride in molten state equal to