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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: aaa777 on April 24, 2008, 11:10:28 AM

Title: REDOX
Post by: aaa777 on April 24, 2008, 11:10:28 AM

hi. thanks for helping me out with my previous chem problems. :) while those problems are over and done with, i have a new one.

we're taking up balancing REDOX reactions in my chem class right now. all the exercises given to us by the teacher were those involving only compounds in aqueous solution. the problem is, our teacher gave us an assignment, 3 items involved compounds in solid state. i would just like to know if there are any implications in the rules regarding balancing when it comes to solid compounds in both acidic and basic.

i'll be waiting for your response. thanks very much.

Title: Re: REDOX
Post by: DevaDevil on April 24, 2008, 11:34:27 AM

obviously in solid state reactions there generally no water present. (and therefore no H₃O⁺ and OH^-, unless in the reactants)
Other than that, balancing rules still apply. One thing to note though: Charge separation is very hard in solids, so if you have ions after reaction, they will be combining to a neutral compound again.

Title: Re: REDOX
Post by: aaa777 on April 24, 2008, 11:51:03 AM

i was given the reaction:

Zn(s) + NO₃^-(aq)  -->  NH₃(aq) + Zn(OH)₄^2-

would the zinc in solid state change the rules of balancing redox for basic?

Edit: corrected tags. Note: (s) and (aq) should be written using normal font size, not subscript. This is defined somewhere in the IUPAC books.

Title: Re: REDOX
Post by: AWK on April 24, 2008, 01:02:49 PM

Zn(s) + NO₃^-(aq)  + OH^- -->  NH₃(aq) + Zn(OH)₄^2-

Balance this reaction

Title: Re: REDOX
Post by: aaa777 on April 24, 2008, 02:21:28 PM

oops. okay! haha:) no change in the rules then.:) thanks so much.