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An acidic solution of Cu²⁺ salt containing 0.4 g of Cu²⁺ is electrolysed until all the copper is deposited. The electrolysis is continued for seven more minutes with the volume of solution kept at 100 ml and the current at 1.2 amp. Calculate the volume of gases evolved at NTP during the entire electrolysis.

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$O_{2}$ = 33.79 m𝑙. $H_{2}$ = 48.45 m𝑙

$O_{2}$ = 87.91 m𝑙. $H_{2}$ = 58.48 m𝑙

$O_{2}$ = 99.79 m𝑙. $H_{2}$ = 58.48 m𝑙

$O_{2}$ = 100 m𝑙. $H_{2}$ = 50 m𝑙

answer is C.

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Detailed Solution

$V_{O_{2}} = \frac{5.6 X 1.2 X 7 X 50}{96500}$

$= 0.029 ltrs$

$= 29 ml$

$V_{H_{2}} = \frac{11.2 X 1.2 X 4 X 60}{96.500}$

$0.05849 ltrs$

$= 5849 ml$

$1 mole of Cu - \frac{1}{2} mole of O_{2} - 11.2 ltrs$

$63.5 g________11.2 ltrs$

$0.4 g_______x$

$x = \frac{0.4}{63.5} X 11.200$

$= 70.5 ml$

$Total of V_{O_{2}} = 29 + 70.5 = 99.5 ml of O_{2}$

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