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An electrochemical cell can generate or use electrical energy. The mass of solid chromium that will be deposited on the electrochemical plate is 7.17 gm.
<h3>What is current?</h3>Current in an electrochemical cell is the ratio of the quantity of electricity in columns and time in seconds.
Given,
Current (I) = 0.350 A
Time = 21.7 hours
Molar mass of chromium = 52.0 g/mol
First time is converted into seconds:
1 hour = 3600 seconds
21.7 hours = 76020 seconds
The quantity of electricity flowing in the electrochemical solution is calculated as:
Electricity required for depositing 1 mole or 52.0 g chromium is calculated as:
In electrochemical solution, chromium chloride is dissociated as:
Two moles of electrons are needed to deposit 52.0 g of chromium.
If, 1 electron = 96500 C
Then, 2 electron = 193000 C
The mass of chromium deposited is calculated as:
193000 C = 52 g chromium
So, 26607 C =
Therefore, 7.17 gm of chromium is produced.
Learn more about an electrochemical cell here:
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