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Topic: Which compound is oxidized and which one reduced in the reaction below?  (Read 1618 times)

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Offline IBM

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Which compound is oxidized and which one reduced in the reaction below?
H3PO3 = H3PO4 + PH3

Offline Babcock_Hall

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Re: Which compound is oxidized and which one reduced in the reaction below?
« Reply #1 on: October 04, 2018, 01:32:52 PM »
Assign oxidation numbers to the atoms.

Offline IBM

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Re: Which compound is oxidized and which one reduced in the reaction below?
« Reply #2 on: October 05, 2018, 11:37:25 AM »
Assign oxidation numbers to the atoms.
H3PO3 (P =+3) = H3PO4 (P =+5) + PH3 (P= -3)

Offline Babcock_Hall

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Re: Which compound is oxidized and which one reduced in the reaction below?
« Reply #3 on: October 05, 2018, 12:28:28 PM »
That looks OK to me.

Offline IBM

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Re: Which compound is oxidized and which one reduced in the reaction below?
« Reply #4 on: October 06, 2018, 02:30:29 AM »
That looks OK to me.
H3PO3 (P =+3) = H3PO4 (P =+5) + PH3 (P= -3)
Could you tell me now which compound is reduced and which compound is oxidized here?

Offline chenbeier

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Re: Which compound is oxidized and which one reduced in the reaction below?
« Reply #5 on: October 06, 2018, 03:25:49 AM »
Learn definition of oxidation: Oxidation is a release of electrons. What does it mean for the oxidation number? Reduction is a acception of electrons, what does it means for the oxidations number?

Offline mjc123

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Re: Which compound is oxidized and which one reduced in the reaction below?
« Reply #6 on: October 08, 2018, 04:50:47 AM »
This is not a standard redox reaction, with an oxidising agent and a reducing agent. It is what is called a disproportionation, in which some of the starting material is oxidised and some is reduced. You start with all P(+3), some of it is oxidised to P(+5) and some reduced to P(-3).
By the way, you should try balancing your equation. Not only the numbers of atoms, but also the oxidation numbers, should balance.

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