got a school prac test coming up in a week, and about the theory i wanna ask: is it possible to have both the anode and the cathode in one beaker in one solution and still produce a voltage? when both electrodes are connected onto one voltmeter will i get a reading? apparently there would be a voltage and it has something to do with displacement.
-
Finished your HSC? Check out our University Discussion, Non-School forums or help out next year's HSC students! -
YOU can help the next generation of students in the community! Share your trial papers and notes on our Notes & Resources page
galvanic cell with one solution? (1 Viewer)
- Thread starter ALL_CAPS
- Start date
strawberrye
Premium Member
Although having both the anode and cathode in one beaker is less usual for galvanic cell, more common for voltaic cells, but if the electrolyte is the same, then yes, it is possible, whether you get a reading or not will depend whether you have correctly connected your electrodes to the -/+ on your voltmeter, if you connected it wrong, you might get a negative voltage-i.e. the voltmeter deflects to less than zero Vs, if this occurs, you know you've made an error, and will most likely have to switch the connections to get a voltage,
Don't confuse things, voltage is basically electric potential energy per unit charge, so it is the NET movement of electrons through the external circuit that you connect with wires to the voltmeter, that creates the reading on the voltmeter, while displacement is essentially referring to the redox reactions-that allows anode become oxidised, convert from metal to metal ions into solutions, cathode being reduced, and the ions making up the electrolyte solution essentially(cations and anions) serving as spectator ions, like in a salt bridge, to preserve ion neutrality and allow the continuous flow of electricity.
Essentially a galvanic cell produces electricity by
1)at anode-oxidation reaction liberates electrons, flow out of the metal of the electrode and into the external circuit
2)these electrons flow through the metallic conductor(wires) of the external circuit to the cathode
3)The reaction at cathode(reduction consumes these electrons)
4)ions migrate through the solution and connecting salt bridge-can be ignored if you want a common solution-to maintain electrical neutrality
Remember for pracs-you must remember validity, reliability, accuracy, how to improve these aspects and evaluate these aspects in reference to prac, remember to draw up a diagram labelled if required, areas for improvement, sources of error-why different from theoretical value(I.e. not performed under standard conditions), independent/dependent/controlled variables may need to be identified-any more questions, welcome to pm me-and best of luck for your upcoming prac
hope my reply helped
Don't confuse things, voltage is basically electric potential energy per unit charge, so it is the NET movement of electrons through the external circuit that you connect with wires to the voltmeter, that creates the reading on the voltmeter, while displacement is essentially referring to the redox reactions-that allows anode become oxidised, convert from metal to metal ions into solutions, cathode being reduced, and the ions making up the electrolyte solution essentially(cations and anions) serving as spectator ions, like in a salt bridge, to preserve ion neutrality and allow the continuous flow of electricity.
Essentially a galvanic cell produces electricity by
1)at anode-oxidation reaction liberates electrons, flow out of the metal of the electrode and into the external circuit
2)these electrons flow through the metallic conductor(wires) of the external circuit to the cathode
3)The reaction at cathode(reduction consumes these electrons)
4)ions migrate through the solution and connecting salt bridge-can be ignored if you want a common solution-to maintain electrical neutrality
Remember for pracs-you must remember validity, reliability, accuracy, how to improve these aspects and evaluate these aspects in reference to prac, remember to draw up a diagram labelled if required, areas for improvement, sources of error-why different from theoretical value(I.e. not performed under standard conditions), independent/dependent/controlled variables may need to be identified-any more questions, welcome to pm me-and best of luck for your upcoming prac
hope my reply helped
anomalousdecay
Premium Member
- Joined
- Jan 26, 2013
- Messages
- 5,766
- Gender
- Male
- HSC
- 2013
HSC 2013, question 12 is the example of the only way in which you can have such a galvanic cell. There is still a voltage produced, with the anode being Zinc, the cathode is Chlorine gas, which produces a reading on the voltmeter.
The voltage has to do with the potential difference caused by moving charges, thus creating this voltage. That is all you need to know in terms of HSC Chemistry.