(a) 0.456 g of a metal gives 0.606 g of its chloride. Calculate the equivalent mass of the metal (b)Calculate the equivalent mass of potassium dichromate. The reduction half-reaction in acid medium is,Cr_(2)O_(7)^(2-)+14H^(+)+6e^(-) rarr 2Cr^(3+)+7H_(2)O

(a) 0.456 g of a metal gives 0.606 g of its chloride. Calculate the eq

1.	(a) 0.456 g of a metal gives 0.606 g of its chloride. Calculate the equivalent mass of the metal (b)Calculate the equivalent mass of potassium dichromate. The reduction half-reaction in acid medium is,Cr_(2)O_(7)^(2-)+14H^(+)+6e^(-) rarr 2Cr^(3+)+7H_(2)O
Answer» Solution :Mass of the METAL = `W_(1)` = 0.456 g. Mass of the metal chloride = `W_(2)` = 0.606 g `:.` Mass of chlorine = `W_(2) -W_(1)` = 0.606 - 0.456 = 0.15 g 0.15 g of chlorine combine with 0.456 g of metal. `:.` 35.46 g of chlorine will combine with`0.456/0.15 xx 35.46` = 107.79 g `EQ ^(-1)`. `Cr_(2)O_(7)^(2-)+14H^(+)+6e^(-) rarr 2Cr^(3+)+7H_(2)O` Equivalent mass = `("Molar mass")/("No. of electrons gained")` `:.` Molar mass of `K_(2)Cr_(2)O_(7)` = 294.18 `:.` Equivalent mass of `K_(2)Cr_(2)O_(7) = 294.18/6 = 49.03`