If a current of 687.6 mA is passed through an electrochemical cell for 56.82 min

Question

If a current of 687.6 mA is passed through an electrochemical cell for 56.82 minutes, what charge, in coulombs, is passed through the cell?

Charge passed through the cell =   .6876 *(56.82*60)= 2344

Suppose that the electrochemical cell consists of two copper electrodes immersed in a copper(II) sulfate solution. At which electrode, anode or cathode, does reduction occur?     

The reduction occurs at the   _______________?

Do you expect that this electrode will increase or decrease in mass as the electrolysis proceeds?

The mass of the electrode will____________?

Calculate the change in the mass of copper at the anode or cathode if the charge calculated above is passed through the cell described. Enter your answer as a positive quantity in mg.

Mass change at the electrode = ____________mg ?

Explanation / Answer

the reduction occurs at cathode

due to reductions positively charged particles are deposited on this electrode so mass of this electrode will increase

now the electrochemical equivalent of copper is 0.0003281 .

so from first law of electrlysis we have m=Z*C=0.0003281*2344=0.76912 gram=769.12 milli gram

so mass change=769.12 milli gram

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.