If I connect a zinc half cell (Left hand side) and a copper half cell (right hand side), I get an E cell value of 1.1V taken from the voltmeter. If I replace the voltmeter with a light bulb, I will get light and heat energy of the bulb.

My question: Will the voltage across the cell remain the same? I mean, the potential difference arises due to the difference in the amount of charge build up on the electrodes... so an electron flows from the zinc electrode to the copper electrode, will the voltage across the bulb decrease?


The electrons are generated by a redox reaction. The zinc metal is oxidised to form a solution of Zn$^{2+}$ ions, and Cu$^{2+}$ ions are reduced to form metallic copper.

$$ Zn \rightarrow Zn^{2+} + 2e $$

$$ Cu^{2+} + 2e \rightarrow Cu $$

So as long as some metallic zinc remains at the anode the voltage will stay the same. Once all the metallic zinc has been dissolved your cell will stop producing a potential difference.

However the voltage will fall when you connect a load, like a light bulb, because the cell has a non-zero internal resistance. If the internal resistance is $R_{int}$ then when you draw a current $I$ the measured voltage will fall by $IR_{int}$.

  • $\begingroup$ So, if I connect a light bulb, there will be a constant voltage across it but the value will be (V-IRint)? $\endgroup$ – Eliza Jan 2 '14 at 13:11
  • $\begingroup$ Yes. The voltage will remain constant until all the zinc has dissolved. $\endgroup$ – John Rennie Jan 2 '14 at 13:48
  • $\begingroup$ Doesn't the potential difference arise due to the difference in the amount of charge build up on the electrodes? Then as the electrons flow from the zinc electrode and zinc is used up, won't the charge on the zinc electrode decrease... and the potential difference should change... I am still confused how the constant voltage arises $\endgroup$ – Eliza Jan 2 '14 at 14:00
  • $\begingroup$ @Eliza: there is no charge buildup. At the cathode metallic Zn is oxidised to Zn$^{2+}$ ions and releases 2 electrons per zinc atom. These electrons flow out of the battery through your bulb and to the anode. There they react with a Cu$^{2+}$ ion and reduce it to form metallic copper. So electrons are produced at the zinc cathode and consumed at the copper anode. The net effect is to dissolve the zinc cathode and precipitate copper at the anode. There is no buildup of electrons. $\endgroup$ – John Rennie Jan 2 '14 at 16:45
  • $\begingroup$ then what causes a potential difference between the electrodes? (i.e. when I connect a voltmeter, there is a reading) $\endgroup$ – Eliza Jan 2 '14 at 16:48

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.