Balbharati solutions for Chemistry [English] 11 Standard chapter 6 - Redox Reactions [Latest edition]

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Oxidation numbers of Cl atoms marked as Cl^a and Cl^b in CaOCl₂ (bleaching powder) are

\[\begin{array}{cc} \ce{Cl^{{a}}}\phantom{.} \\/\phantom{...} \\ \ce{Ca}\phantom{......} \\ \backslash\phantom{..} \\\phantom{........} \ce{O-Cl^{{b}}}\phantom{.} \end{array}\]

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Which of the following is not an example of redox reaction?

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A compound contains atoms of three elements A, B, and C. If the oxidation state of A is +2, B is +5 and that of C is -2, the compound is possibly represented by

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The coefficients p, q, r, s in the reaction \[\ce{{p}Cr2O7^{2Θ} + {q}Fe^{2⊕}->{r}Cr^{3⊕} + {s}Fe^{3⊕} + H2O}\] respectively are:

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For the following redox reactions, find the correct statement.

\[\ce{Sn^{2⊕} + 2Fe^{3⊕}->Sn^{4⊕} + 2Fe^{2⊕}}\]

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Oxidation number of carbon in H₂CO₃ is

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Which is the correct stock notation for manganese dioxide?

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Oxidation number of oxygen in superoxide is

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Which of the following halogens does always show oxidation state -1?

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The process \[\ce{SO2->S2Cl2}\] is

Write the formula for the following compound:

Mercury(II) chloride

Write the formula for the following compound:

Thallium(I) sulphate

Write the formula for the following compound:

Tin(IV) oxide

Write the formula for the following compound:

Chromium(III) oxide

In which chemical reaction does carbon exhibit variation of oxidation state from - 4 to + 4? Write a balanced chemical reaction.

In which reaction does nitrogen exhibit variation of oxidation state from –3 to +5?

Calculate the oxidation number of the underlined atom.

H₂SO₄

Calculate the oxidation number of the underlined atom.

HNO₃

Calculate the oxidation number of the underlined atom.

H₃PO₃

Calculate the oxidation number of the underlined atom.

K₂C₂O₄

Calculate the oxidation number of the underlined atom.

H₂S₄O₆

Calculate the oxidation number of the underlined atom.

Cr₂O₇²⁻

Calculate the oxidation number of the underlined atom.

NaH₂PO₄

Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.

\[\ce{2Cu2O_{(S)} + Cu2S_{(S)}->6Cu_{(S)} + SO2_{(g)}}\]

Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.

\[\ce{HF_{(aq)} + {OH}^-_{ (aq)}->H2O_{(l)} + {F}^ -_{ (aq)}}\]

Justify that the following reaction is redox reaction; identify the species oxidized/reduced, which acts as an oxidant and which acts as a reductant.

\[\ce{I2_{(aq)} + 2S2O^{2-}_{3(aq)}->S4O^{2-}_{6(aq)} + 2I^-_{ (aq)}}\]

What is oxidation?

Identify the following pair of species is in its oxidized state.

Mg/Mg²⁺

Identify the following pair of species is in its oxidized state?

Cu/Cu²⁺

Identify the following pair of species is in its oxidized state?

\[\ce{O2/O^2-}\]

Identify the following pair of species is in its oxidized state?

Cl₂/Cl⁻

Justify the following reaction as a redox reaction.

\[\ce{2Na_{(s)} + S_{(s)}->Na2S_{(s)}}\]

Find out the oxidizing and reducing agents.

Provide the stock notation for the following compound:

HAuCl₄

Provide the stock notation for the following compound:

Tl₂O

Provide the stock notation for the following compound:

FeO

Provide the stock notation for the following compound:

Fe₂O₃

Provide the stock notation for the following compound:

MnO

Provide the stock notation for the following compound:

CuO

Assign oxidation number atom in the following species.

\[\ce{Cr(OH)^Θ_4}\]

Assign oxidation number atom in the following species.

Na₂S₂O₃

Assign oxidation number atom in the following species.

H₃BO₃

Which of the following redox couple is a stronger oxidizing agent?

Cl₂ (E⁰ = 1.36 V) and Br₂ (E⁰ = 1.09 V)

Which of the following redox couple is a stronger oxidizing agent?

\[\ce{MnO^Θ_4}\](E⁰ = 1.51 V) and \[\ce{Cr2O^{2Θ}_7}\](E⁰ = 1.33 V)

Which of the following redox couple is a stronger reducing agent?

Li (E⁰ = - 3.05 V) and Mg (E⁰ = - 2.36 V)

Which of the following redox couple is a stronger reducing agent?

Zn (E⁰ = - 0.76 V) and Fe (E⁰ = - 0.44 V)

Balance the following reaction by oxidation number method.

\[\ce{Cr2O^2-_{7(aq)} + SO^2-_{3(aq)}->Cr^3+_{ (aq)} + SO^2-_{4(aq)}(acidic)}\]

Balance the following reaction by oxidation number method.

\[\ce{MnO^-_{4(aq)} + Br^-_{ (aq)}->MnO2_{ (s)} + BrO^-_{3(aq)}(basic)}\]

Balance the following reaction by oxidation number method.

\[\ce{H2SO4_{(aq)} + C_{(s)}->CO2_{(g)}  + SO2_{(g)} + H2O_{(l)}(acidic)}\]

Balance the following reaction by oxidation number method.

\[\ce{Bi(OH)_{3(s)} + Sn(OH)^-_{3(aq)}->Bi_{(s)}  + Sn(OH)^2-_{6(aq)}(basic)}\]

Balance the following redox equation by half-reaction method.

\[\ce{H2C2O_{4(aq)} + MnO^-_{4(aq)}->CO2_{(g)} + Mn^2+_{( aq)}(acidic)}\]

Balance the following redox equation by half-reaction method.

\[\ce{Bi(OH)_{3(s)} + SnO^2-_{2(aq)}->SnO^2-_{3(aq)} + Bi^_{(s)}(basic)}\]

Complete the following table:

Assign oxidation number to the underlined species and write Stock notation of compound