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0.222g Of A Divalent Metal Is Deposited When A Current Of 0.45 Amperes Is Passed Through A Solution Of It’s Salt For 25 Minutes Using Appropriate Electrodes. Calculate The Relative Atomic Mass Of The Metal. (1 Faraday =96500c/mol)

Posted on October 20, 2022 by admin

0.222 g of a divalent metal is deposited when a current of 0.45 amperes is passed through a solution of its salt for 25 minutes using suitable electrodes. Calculate the relative atomic mass of the metal. (1 Faraday = 96500c/mol) I need the whole answer Pls I need the whole 63.5 resolution tyet Please I need the whole question answer and resolution thanks Many thanks sir How many coulombs were used? It’s coulombs = amps x seconds = 0.45 A x 25 min x 60 sec/min = about 700 but you need a better answer than that estimate.

96,500 coulombs will deposit (atomic mass/2) grams of divalent metal. So

(atomic mass/2) x (700/96,500) = 0.222g

Solve the atomic mass. am a student pls i need to solve all this question Thanks. Awesome I need all the work

Am a learner love you ❤️

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