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Stoichiometry & Redox Reaction Test - 4
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Stoichiometry & Redox Reaction Test - 4

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  • Question 1/10
    1 / -0

    The reaction 2KClO3 → 2KCl + 3 O2 is

    Solutions

    The given reaction is an intramolecular redox change.

     

  • Question 2/10
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    The mass of H2O2 that is completely oxidised with 31.2 g of KMnO4 (molar mass = 158 g mol–1) in acidic medium is

    Solutions

     

  • Question 3/10
    1 / -0

    For the reaction between KMnO4 and H2O2, the number of electrons transferred per mole of H2O2 is

    Solutions

    KMnO4 is a stronger oxidising agent than H2O2 in the acidic, basic as well as neutral mediums.
    In the neutral medium,
    2KMnO4 + 3H2O2 → 2MnO2 + 2KOH + 2H2O + 3O2
    The overall equation involves a transfer of 6 electrons.
    Therefore, the number of electrons transferred per mole of H2O2 is 2 and the number of electrons transferred per mole of KMnO4 is 3.

     

  • Question 4/10
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    In acidic medium, dichromate ion oxidises ferrous ion to ferric ion. If the gram molecular weight of potassium dichromate is 294 g, its gram equivalent weight is

    Solutions

    The reaction of dichromate ion with ferrous ion in acidic medium takes place as follows:

     

  • Question 5/10
    1 / -0

    If equal volumes of 1 M KMnO4 and 1 M K2Cr2O7 solutions are allowed to oxidise Fe (II) to Fe (III) in acidic medium, then Fe (II) oxidisation

    Solutions

    Equal volumes of 1 M KMnO4 and 1 M K2Cr2O7 have equal number of moles of KMnO4 and K2Cr2O7.
    As 1 mole of KMnO4 accept 5 moles of electrons and 1 mole of K2Cr2O7 accepts 6 moles of electrons, K2Cr2O7 will oxidise more Fe2+ to Fe3+.

     

  • Question 6/10
    1 / -0

    Which of the following reactions involves both oxidation and reduction?

    Solutions

    The reaction in which the oxidation number of elements changes will involve oxidation and reduction.
    Write the oxidation number of each of the elements in reactant and product molecules to find the answer.

     

  • Question 7/10
    1 / -0

    In the reaction HAsO2 + Sn2+ → As + Sn4+ + H2O, the oxidising agent is

    Solutions

    Oxidising agent itself undergoes reduction during a redox reaction.

    ∴

    Oxidation state of As in HAsO2 is x.
    ∴ 1 + x + (2x - 2) = 0
    or x = 3
    Oxidation state of As = 0
    Oxidation state of Sn in Sn2+ = +2
    Oxidation state of Sn in Sn4+ = + 4

    ∵ Increase in the oxidation number is oxidation.
    ∵ Sn2+ is oxidised to Sn4+ during the reaction and it is the reducing agent.
    ∵ Decrease in the oxidation number is reduction.
    ∵ HAsO2 is reduced to As and it is the oxidising agent.

     

  • Question 8/10
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    Consider the reaction between potassium permanganate and a metal sulphite represented as follows.

    Which of the following options about the process is correct?

    Solutions

    The balanced equation shows that 1 mole of potassium permanganate will oxidise 2.5 moles of the metal sulphite.

    There is a net transfer of 10 electrons during the complete reaction.

    Only 8 mL of KMnO4 solution would be required to neutralise a 20 mL equimolar solution of metal sulphite.

     

  • Question 9/10
    1 / -0

    The standard values of A, B and C are +0.68 V, -2.54 V and -0.50 V, respectively. Which of the following statements is correct in context to the given data?

    Solutions

    Substances with a lower value of reduction potential are stronger reducing agents.
    Therefore, the increasing order of reducing strengths is A < C < B.
    The increasing order oxidising strengths is B < C < A.
    Hence, B can be oxidised by both A and C.

     

  • Question 10/10
    1 / -0

    The standard reduction potentials of Fe+2/Fe and Cu+2/Cu electrodes are -0.44 and 0.34 volts, respectively.

    Which of the following statements is true?

    Solutions

    Since copper has a higher reduction potential than iron, the following redox reaction will be spontaneous:

     

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