1. Assuming that your identification of the unknown metal is correct, write the

Question

1. Assuming that your identification of the unknown metal is correct, write the specific half-reaction that occured at the anode for your metal in this experiment? (my metal was Nickel)

2. If aluminum metal had been your unknown, and the same amount of hydrogen gas had been released, what mass of aluminum could have been oxidized at the anode?

3. Calculate the average electric current that flowed during this expreiment. Assume that the two runs of your experiment lasted 15 minutes each. You should be able to find the total amount of electric charge that flowed during the experiment from your data and calculations.

4. Calculate the number of coulombs of electric charge on a single electron, given Faraday's number provided in question #3 and Avogadro's number.

Explanation / Answer

(1) Anodic Half Reaction: Ni (s) -------------> Ni2+ (aq.) + 2 e

(2) 3 mol of H2 requires 2 mol of Al

Then 1 mol of H2 requires 2/3 mol of Al = 0.67 mol Al = 0.67*27 = 18.09 g. of Al

(4) 1 mole of electron have a charge of 96500 C

then one electron can have a charge of 96500/(6.022*1023) =1.602 x 10 -19 C

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