At 7:12 will I get the marks if I balanced the equations because each half cell has a different number of electrons? I wrote down: 2Mn^2+, 8H2O, 10Fe^3+ and 5Br2 Basically I imaged that all three half cells were redoxing together so I had to make sure the electrons matched from the data in the question. And for the last question would hydrogen being more volatile/explosive because it’s a gas compared to Methanol being a liquid be a valid answer? Thanks
Hi there, for question 1a i, I was just wondering if the iron half cell should be drawn on the left because it has a more negative (less positive) electrode potential compared to the silver half cell?
Hi my favourite geordie teacher. Thanks for the video, I have a question regarding 3:56 . Could you tell me the specific rule please as to whats making the reaction go in that direction, in terms of le chateliers. Thanks again, Daniel
If you increase the concentration of any reactant, an equilibrium will shift in the forwards direction to minimise the change. Because of this, the standard electrode potential increases
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Hi sir could you do a quick explanation on the effect of increasing conc on the cell potential as I didn't quite get q1 a ii
why are you using a silver electrode for the silver solution but a platinum electrode for the iron solution
The two oxidation states for the iron are the two ions in the solution
At 7:12 will I get the marks if I balanced the equations because each half cell has a different number of electrons?
I wrote down: 2Mn^2+, 8H2O, 10Fe^3+ and 5Br2
Basically I imaged that all three half cells were redoxing together so I had to make sure the electrons matched from the data in the question.
And for the last question would hydrogen being more volatile/explosive because it’s a gas compared to Methanol being a liquid be a valid answer? Thanks
very useful thank you!
Really well explained sir, thank you !
Most welcome!
Hi there, for question 1a i, I was just wondering if the iron half cell should be drawn on the left because it has a more negative (less positive) electrode potential compared to the silver half cell?
OCR does not insist on this so I don’t bother
@@MaChemGuy ah ok thank you!
@@angelahalton8827 You are right btw :)
Hi my favourite geordie teacher.
Thanks for the video, I have a question regarding 3:56 .
Could you tell me the specific rule please as to whats making the reaction go in that direction, in terms of le chateliers.
Thanks again,
Daniel
Hi does anyone know?
If you increase the concentration of any reactant, an equilibrium will shift in the forwards direction to minimise the change. Because of this, the standard electrode potential increases
Why does the voltage become more positive when the Ag+ concentration is increased?
Equilibrium shifts to the right