flipping equations

[Ghadir Seder 1G]

How do you know which equation to flip so that the electrons cancel out? Is it the reduction or oxidation equation that you flip?

[chimerila]

I'm still kind of confused on that too. I just know that to cancel the electrons out, make sure whatever you end up flipping, you're reduction equation has electrons on the left, and the oxidized equation has electrons on the right

[Kimberly Koo 2I]

This would depend on the situation given, but generally, you would want to manipulate the equations so that you end up with the standard potential of the cell being positive (the reaction is spontaneous). Use the equation E(cell)=E(electrode on right of cell diagram)-E(electrode on left of cell diagram)

[vpena_1I]

If I'm understanding your question correctly, you would flip the oxidation one, so that your electrons are on the right side of the equation, and on your left for the reduction half reaction.

[Chris Charton 1B]

The E(cell) has to be positive, so the cathode will always be the larger (more positive) reduction potential value, and the anode will then "be flipped" so that it is giving off an electron (oxidized).

[Micah3J]

What are you guys referring to as "flipping"? Does this mean making one side negative or like looking at the reverse reaction instead?

[SMIYAZAKI_1B]

The wording is definitely a little difficult to understand but I am also assuming that you are asking us for which redox hzlf equation to switch the product and reactant sides. I would say that generally, you would want to have the cell potential to be positive in order to allow the system to have spontaneous reaction.

[905373636]

This is all based on the equation that Ecell = Eright - Eleft and as Eleft is the oxidation cell, you 'flip' the oxidation cell.