1. Not finding help here? Sign up for a free 30min tutor trial with Chegg Tutors
    Dismiss Notice
Dismiss Notice
Join Physics Forums Today!
The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

Having difficulty with Ox-Redox

  1. Nov 27, 2007 #1

    Can someone please explain to me something here please? In this oxidation problem

    Na2Cr2O7 + HNO3 + Na2SO3 yields NaNO3 + Cr(NO3)3 + Na2SO4 + H2O

    I know S is Oxidized and Cr is Reduced. However, when I look at the solution set, I am get completely confused.

    They are putting

    SO3^2- yields SO4^2- for oxidation and for reduction they have Cr2O7^2- yields 2 Cr ^ 3+.

    I understand how to get what is Oxidized and what is reduced.

    However, I am having trouble knowing what to eliminate. How can they just get read of the Na2 in the first one and (NO3)3 in the second one? Is there some sort of rule that tells you what you can get rid of? Also, once they do get rid of half of the original ion, how do they assign the charge? Is the charge just the polyatomic charge of sulfite and sulfate?

    Thanks in advance
  2. jcsd
  3. Nov 27, 2007 #2
    open second review, it seems that they seperated polyatomic ions from the main elements. is this possible? and would you follow this step for other ox redox reactions?
  4. Nov 27, 2007 #3


    User Avatar
    Staff Emeritus
    Science Advisor
    Gold Member

    Write down each compound as a sum of its "ionic" species (example: [itex]Na_2Cr_2O_7 = 2Na^+ + Cr_2O_7^{2-}[/itex]). Then you just throw away all the ions that do not change their oxidation states (example: [itex]Na^+, NO_3^-, H^+)[/itex].
  5. Nov 27, 2007 #4
    So would this turn out to be:

    2 Na + Cr2O7^2- + H + NO3 2- + 2 Na + SO3 ^ 2- yields Na + NO3 + Cr(NO3)3 + 2 NA + SO4 ^ 3 + H2O

    and when you refer to "ionic" species, what are you referring to exactly?

    Thanks for the help
    Last edited: Nov 27, 2007
  6. Nov 28, 2007 #5


    User Avatar
    Staff Emeritus
    Science Advisor
    Gold Member

    I mean that you have to include the charges on all species.

    Na and H should both have a charge of 1+ (or simply +). Also, the charge on the nitrate ion (NO3) is 1-, not 2-.

    And finally, you have yet to split up Cr(NO3)3 into its parts.
  7. Nov 28, 2007 #6
    I think I am beginning to understand this now.

    1. Assign ox states, see what is oxidized and what is reduced.

    2. "Split the elements", but if it is a polyatomic ion, you keep that together.

    In this problem, you would split

    Na2Cr2O7 into 2Na^+1 + 2Cr^6 + 7O^-2.

    Then you would split HNO3 into H^+1 + NO3^-1.

    Disregarding this problem, should you also keep all Oxygen's next to an element?

    For Instance:

    I2 + HNO3 -------> NaIO3 + NO3

    I is oxidized and N is reduced.

    would the equation for I be I2 ---------> I03

    and for N be NO3^1 ---------> Na^+1.

    Thanks in advance
Know someone interested in this topic? Share this thread via Reddit, Google+, Twitter, or Facebook

Have something to add?

Similar Discussions: Having difficulty with Ox-Redox
  1. Redox reaction (Replies: 1)

  2. RedOx formula (Replies: 1)

  3. Redox equilibrium (Replies: 0)

  4. Redox Reactions (Replies: 4)