Chegg Write the balanced half-reactions for the following oxidation-reduction reaction that occurs in acid solution. Determine the number of

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Chegg Write the balanced half-reactions for the following oxidation-reduction reaction that occurs in acid solution. Determine the number of electrons that appears in the balanced half reactions. Number of electrons

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Edana Edana 5 years 2021-07-18T17:23:49+00:00 1 Answers 69 views 0

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  1. King
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    2021-07-18T17:25:30+00:00
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    Answer:

    Reduction half-reaction: Cr₂O₇²- (aq) + 14H+ (aq) + 6e- —-> 2Cr³+ (aq) + 7 H₂O (l)

    Oxidation half-reaction: 6 Cl- (aq) —> 3 Cl₂ (g) + 6e-

    Number of electrons = 6 electrons

    Note: The question is incomplete. A similar but complete question is given below :

    Write the balanced half-reactions for the following oxidation-reduction reaction that occurs in acid solution. Determine the number of electrons that appears in the balanced half reactions.

    Cr₂0₇²- (aq) + CI- (aq) —> Cr³+ (aq) + Cl₂(g)

    Number of electrons =

    Explanation:

    A redox reaction is a reaction in which both oxidation and reduction occur simultaneously and to to the same extent.

    Oxidation involves a loss of electron by atom of an element while reduction involve a gain of electrons.

    A redox reaction can be split into two half-reaction; a reduction half-reaction andan oxidation half-reaction. The half-reactions in the given redox reaction is balanced as follows below:

    Reduction half-reaction: Cr⁶+ being reduced to Cr³+

    Cr₂O₇²- (aq) —> Cr³+ (aq)

    Since the reaction takes place in acidic medium, H+ and H₂O is added to the left and right-hand side of the equation respectively in order to balance the atoms

    Cr₂O₇²- (aq) + 14H+ (aq) —-> 2Cr³+ (aq) + 7 H₂O (l)

    Since 3 electrons are gained by Cr⁶+ in being reduced to Cr³+, 2 molecules of Cr⁶+ will accept 3 electrons each to give a total of 6 electrons

    Cr₂O₇²- (aq) + 14H+ (aq) + 6e- —-> 2Cr³+ (aq) + 7 H₂O (l)

    Oxidation half-reaction: Cl- ions are oxidized to Cl₂

    Cl- (aq) —> Cl₂

    Two Cl- will each lose an electron to form Cl₂. Since the number of electrons gained in the reduction half-reaction is six, six electrons must be lost here as well. Therefore, the electrons involved and the number of moles of atoms involved are balanced as follows:

    6 Cl- (aq) —> 3 Cl₂ (g) + 6e-

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