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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: winspice on August 22, 2010, 03:22:29 PM

Title: balancing redox equation
Post by: winspice on August 22, 2010, 03:22:29 PM

ReO2 + Cl2  ---->   HReO4 + Cl-
Cl2 ----> Cl-

I need some help in balancing this redox equation.I don't know if I should combine the Cl- and H+ at the end or should I add OH- instead? Thanks.

Title: Re: balancing redox equation
Post by: Borek on August 22, 2010, 03:26:18 PM

Are you told what is solution pH, or not?

Title: Re: balancing redox equation
Post by: winspice on August 22, 2010, 04:06:55 PM

no pH is provided.

Title: Re: balancing redox equation
Post by: Borek on August 22, 2010, 04:18:39 PM

So start with water on the left.

Try to write both half reactions at first. Can you tell what is getting oxidized and what is getting reduced?

Title: Re: balancing redox equation
Post by: winspice on August 22, 2010, 04:24:49 PM

Cl2 is going to be reduced while ReO2 is oxidized. At the end I came up with the equation
3Cl2+2ReO2+4H2O--->6Cl-+6H+ +2HReO4

Title: Re: balancing redox equation
Post by: Borek on August 22, 2010, 05:11:32 PM

Seems OK.