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AS Chemistry - Redox

Lead(IV) oxide, PbO2, reacts with concentrated hydrochloric acid to produce chlorine, lead(II) ions, Pb2+,and water.

(i) Write a half-equation for the formation of Pb2+ and water from PbO2 in the presence of H+ ions.
(ii)Write a half-equation for the formation of chlorine from chloride ions.
(iii) Hence deduce an equation for the reaction which occurs when concentrated hydrochloric acid is added to lead(IV) oxide, PbO2

Please help :smile:
Reply 1
For part (i), I got
PbO2 + 4H+ β†’ Pb2+ + 2H2O + 2e-

The mark scheme says:
PbO2 + 4H+ + 2eβˆ’ β†’ Pb2+ + 2H2O

I don't understand why the electrons are on the other side. Can someone please explain?
Original post by 010534
For part (i), I got
PbO2 + 4H+ β†’ Pb2+ + 2H2O + 2e-

The mark scheme says:
PbO2 + 4H+ + 2eβˆ’ β†’ Pb2+ + 2H2O

I don't understand why the electrons are on the other side. Can someone please explain?


What's the oxidation state of Pb in PbO2? How about Pb2+? Does this help? :smile:
Tips:
to balance a redox equation firstly u balance the oxygen with water, then balance the hydrogens in water with H+ then balance the charges on both sides

or u can balance the charges on Pb first with electrons then only oxygen with water then hydrogens in water with H+
Reply 4
Original post by 010534
For part (i), I got
PbO2 + 4H+ β†’ Pb2+ + 2H2O + 2e-

The mark scheme says:
PbO2 + 4H+ + 2eβˆ’ β†’ Pb2+ + 2H2O

I don't understand why the electrons are on the other side. Can someone please explain?


I am not sure if this will make sense but here goes:

In PbO2, the oxidation state of the lead is +4, because the overall oxidation state of PbO2 is 0 because charges cancel out, leaving a compound neutral. The oxidation state of O is always -2, and there are two oxygen atoms here, so the charge on the O2 is -4. Therefore to make PbO2 0, the oxidation number of Pb must be +4.

If something has a charge of +4, this means that it has lost 4 electrons, right? (think about sodium as an ion - Na+) So surely in order to become Pb2+, it has to have lost 2 electrons. This means that it has to have gained 2 electrons in order to become Pb2+ on the other side of the equation.

And it's the PbO2 that has to have gained 2 electrons in order to become Pb2+, because if you think about it, if the + 2e- was on the other side of the equation, that would be equivalent to the PbO2 losing two electrons, which would not make Pb2+, but Pb6+, which isn't what you want as a product.

Hope that helps - please reply if that explanation was ok :smile:
(edited 8 years ago)
Reply 5
Original post by sue99
I am not sure if this will make sense but here goes:

In PbO2, the oxidation state of the lead is +4, because the overall oxidation state of PbO2 is 0 because charges cancel out, leaving a compound neutral. The oxidation state of O is always -2, and there are two oxygen atoms here, so the charge on the O2 is -4. Therefore to make PbO2 0, the oxidation number of Pb must be +4.

If something has a charge of +4, this means that it has lost 4 electrons, right? (think about sodium as an ion - Na+) So surely in order to become Pb2+, it has to have lost 2 electrons. This means that it has to have gained 2 electrons in order to become Pb2+ on the other side of the equation.

And it's the PbO2 that has to have gained 2 electrons in order to become Pb2+, because if you think about it, if the + 2e- was on the other side of the equation, that would be equivalent to the PbO2 losing two electrons, which would not make Pb2+, but Pb6+, which isn't what you want as a product.

Hope that helps - please reply if that explanation was ok :smile:


Yes! Thank you very much! So it's because of the charges needing to balance :smile:
Reply 6
Original post by SeanFM
What's the oxidation state of Pb in PbO2? How about Pb2+? Does this help? :smile:


Thank you :smile: It helped a lot^^
Does anyone know what part three of this question is??? I'm so stuck πŸ˜₯
Reply 8
Original post by Gracie jewel
Does anyone know what part three of this question is??? I'm so stuck πŸ˜₯


I got PbO2 + 2Cl- + 4H+ --> Pb2+ + 2H2O + Cl2 by adding the two half equations together since HCl provides Cl- ions and H+ ions
Original post by 010534
For part (i), I got
PbO2 + 4H+ β†’ Pb2+ + 2H2O + 2e-

The mark scheme says:
PbO2 + 4H+ + 2eβˆ’ β†’ Pb2+ + 2H2O

I don't understand why the electrons are on the other side. Can someone please explain?


the electrons are on the other side as this reaction is a REDUCTION reaction, electrons are ADDED therefore should be on the left side.
Reply 10
Original post by Kevin De Bruyne
What's the oxidation state of Pb in PbO2? How about Pb2+? Does this help? :smile:


ik this was 7 years ago but do you remember where you got the mark scheme from?

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