username3835832
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#1
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#1
http://pmt.physicsandmathstutor.com/...Potentials.pdf

question 4b,
in the second equation Cr2O7 2– acts as a oxidising agent and gets reduced.
forming Cr 3+.
Can Cr 3+ also act as an oxidising agent?
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charco
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#2
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(Original post by chemquestion)
http://pmt.physicsandmathstutor.com/...Potentials.pdf

question 4b,
in the second equation Cr2O7 2– acts as a oxidising agent and gets reduced.
forming Cr 3+.
Can Cr 3+ also act as an oxidising agent?
Only with species that are stronger reducing agents. For example, it would react with magnesium forming chromium and oxidise the magnesium to Mg2+

There is also the possibility of forming chromium(II) in certain cases.
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#3
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(Original post by charco)
Only with species that are stronger reducing agents. For example, it would react with magnesium forming chromium and oxidise the magnesium to Mg2+

There is also the possibility of forming chromium(II) in certain cases.
So it depends on the electrode potential?
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charco
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(Original post by chemquestion)
So it depends on the electrode potential?
yes
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#5
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#5
http://pmt.physicsandmathstutor.com/...Potentials.pdf

question 5bii do all the ions in the both equations go into the solution when we label the diagram?
so for this equation VO2+ + 2H+ + e– V3+ + H2O
we have to include VO2+ 2H+ and V3+ , when labelling the half-cell?
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#6
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(Original post by chemquestion)
http://pmt.physicsandmathstutor.com/...Potentials.pdf

question 5bii do all the ions in the both equations go into the solution when we label the diagram?
so for this equation VO2+ + 2H+ + e– V3+ + H2O
we have to include VO2+ 2H+ and V3+ , when labelling the half-cell?
One redox couple goes into one half-cell and the other redox couple into the other half-cell. If they are in direct contact there would be no reason for electricity to flow around the external circuit.
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