The electrolysis of TℓBr3 at high temperature produces thallium metal. If a constant electrical current of 10.00 × 103?? flows for exactly two hours, calculate the number of thallium atoms present in the metal produced during this time.
The balanced equation for a voltaic cell is as follows:
2NO3-(aq)+8H3O+(aq)+3Ca(s) -> 2NO (g) + 3Ca2 (aq) + 12 H2O (l)
In one half-cell (containing a graphite electrode) the following conditions apply:
[NO3- ] = 0.200 M; PNO = 0.100 atm; pH = 2.000
This is combined with a standard Ca2+ǀCa half-cell.
Under these conditions, the cell potential was measured to be 3.678 V at 250 'C.
By calculating the value of the reaction quotient and Ecell 0 under these conditions, determinethe value of the standard potential for the Ca2+ ǀ Ca half-cell.
2.2 The
thallium atoms present in the metal produced during this time.
Please only answer Question 2.2
Given:
Current (I) = 10.00 x 103 Amp
Time(t) = 2 hour = 7200 sec
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