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.
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:
[tex]\begin{aligned} \rm Q & = \rm It\\\\& = 0.350 \times 76020 \\\\& = 26607\;\rm C \end{aligned}[/tex]
Electricity required for depositing 1 mole or 52.0 g chromium is calculated as:
In electrochemical solution, chromium chloride is dissociated as:
[tex]\rm CrCl_{2} \rightarrow Cr^{2+} + 2 Cl^{-} \\\\\rm Cr^{2+} +2 e^{-} \rightarrow Cr[/tex]
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 = [tex]\dfrac{26607 \times 52}{193000} = 7.17 \;\rm gm[/tex]
Therefore, 7.17 gm of chromium is produced.
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