Chromium metal can be plated out from an acidic solution containing CrO_(3) according to the following the reaction: CrO_(3) + 6H^(+) + 6e^(-) rarr Cr + 3H_(2)O How long will it take to plate out 1.5 gm of Cr using 12.5 ampere current ? (Atomic weight of Cr =52, 1F =96500 C)
How many grams of Cr are deposited in the electrolysis of solution of Cr (NO_3)_3 in the same time that it takes to deposite 0.54g of Ag in a silver coulometer arranged in series with the Cr(NO_3)_3 cell? (Atomic mass: Cr=52.0,Ag=108)
How many moles of Cr are there in 85 g of Cr_(2) S_(3) ? (Cr = 52 , S = 32 )
Calculate how long it will take to deposit 1.0 g of chromium when a current of 1.25 . A flows through a solution of chromium (III) sulphate . (Molar mass of Cr = 52).
Chromium metal can be plated out from an acidic solution containing CrO_(3) according to the following equation : CrO_(3)(aq)+6H^(o+)+6H^(o+)(aq)+6e^(-) rarr Cr(s)+3H_(2)O a. How many grams of chromium will be plated out by 24000C ? b. How long will take to plate out 1.5g of chromium by using 12.5 A current ?
