The chemical equivalent of copper and zinc are 32 and 108 respectively- When copper and silver voltameter are connected in series and electric current is passed through sometimes- 1-6 g of copper is deposited- Then- the mass of silver deposited will be

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Toppr Admin · Accepted Answer

Correct option is C- 5-4 gFrom Faraday-8217-s law- m-E - constantwhere m - mass of substance deposited- E -chemical equivalent- - -therefore -dfrac-m-2-m-1- - -dfrac-E-2-E-1- -Rightarrow-160- m-2- - -dfrac-108-32- -times 1-6 - 5-4g -

The chemical equivalent of copper and zinc are 32 and 108 respectively. When copper and silver voltameter are connected in series and electric current is passed through for sometimes, 1.6 g of copper is deposited. Then, the mass of silver deposited will be

Correct option is C. 5.4 g
From Faraday’s law, m/E = constant
where m = mass of substance deposited, E =chemical equivalent. $$ \therefore \dfrac{m_{2}}{m_{1}} = \dfrac{E_{2}}{E_{1}} \Rightarrow m_{2} = \dfrac{108}{32} \times 1.6 = 5.4g $$

The chemical equivalent of copper and zinc are 32 and 108 respectively. When copper and silver voltameter are connected in series and electric current is passed through for sometimes, 1.6 g of copper is deposited. Then, the mass of silver deposited will be

Correct option is C. 5.4 gFrom Faraday’s law, m/E = constantwhere m = mass of substance deposited, E =chemical equivalent. $$ \therefore \dfrac{m_{2}}{m_{1}} = \dfrac{E_{2}}{E_{1}} \Rightarrow m_{2} = \dfrac{108}{32} \times 1.6 = 5.4g $$

Correct option is C. 5.4 g
From Faraday’s law, m/E = constant
where m = mass of substance deposited, E =chemical equivalent. $$ \therefore \dfrac{m_{2}}{m_{1}} = \dfrac{E_{2}}{E_{1}} \Rightarrow m_{2} = \dfrac{108}{32} \times 1.6 = 5.4g $$