Balancing redox reactions in question 14.13

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Kevin Tabibian 1A
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Balancing redox reactions in question 14.13

Postby Kevin Tabibian 1A » Mon Mar 12, 2018 3:53 pm

For part d of question 14.13, where you are asked to write the half reactions of (d) Au(+) → Au + Au(3+), how do we know that one of the half-reactions is Au → Au(3+) + 3e instead of Au(+) → Au(3+) + 2e. I assumed that both half reactions would begin with Au(+), how should I have known that one was going to begin with Au instead?

Victoria Draper 1G
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Re: Balancing redox reactions in question 14.13

Postby Victoria Draper 1G » Mon Mar 12, 2018 8:16 pm

For this question you have to make sure that the sum of the two half reactions cancels out certain products and reactants in order to give you the original reaction equation. If both half reactions began with Au(+) then the sum of the two half reactions would not give you the reaction equation of Au(+) → Au + Au(3+).

mayapartha_1D
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Re: Balancing redox reactions in question 14.13

Postby mayapartha_1D » Tue Mar 13, 2018 7:20 pm

Hi!

Simply writing out the half reactions will make it a lot easier! I always make sure to write out the half-reactions that are given and make sure they cancel out electrons to become the final reaction. As Victoria stated, making sure that the electrons cancel is the easiest way to balance the reaction.


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