The element that does not show a disproportionation tendency is/are:

1. Cl

2. Br

3. F

4. I

Subtopic:  Oxidizing & Reducing Agents |
 83%
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Assertion (A): In the presentation 
\( \mathrm{E}_{\mathrm{Fe}^{3+}}^{\ominus} /_{ \mathrm{Fe}^{2+}}\) \( \text { and } \mathrm{E}_{\mathrm{Cu}^{2+}}^{\ominus} / _{\mathrm{Cu}^{\prime}} \mathrm{Fe}^{3+} / \mathrm{Fe}^{2+} \) and\(\text { } \mathrm{Cu}^{2+} / \mathrm{Cu}\) are reodox couples
Reason (R): A redox couple is the combination of the oxidised and reduced forms of a substance involved in an oxidation or reduction half cell.
 
1. Both (A) and (R) are True and (R) is the correct explanation of (A).
2. Both (A) and (R) are True but (R) is not the correct explanation of (A).
3. (A) is True but (R) is False.
4. (A) is False but (R) is True.
Subtopic:  Introduction to Redox and Oxidation Number |
 74%
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Given below are two statements: 

Assertion (A): The decomposition of hydrogen peroxide to form water and oxygen is an example of a disproportionation reaction.
Reason (R): The oxygen of peroxide is in –1 oxidation state and it is converted to zero oxidation state in O2
and –2 oxidation state in H2O.

1. Both (A) and (R) are true and (R) is the correct explanation of (A).
2. Both (A) and (R) are true but (R) is not the correct explanation of (A).
3. (A) is true but (R) is false.
4. (A) is false but (R) is true.

Subtopic:  Redox Titration & Type of Redox |
 89%
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Which of the following is not an example of redox reaction?

1. CuO+H2Cu+H2O

2. Fe2O3+3CO2Fe+3CO2

3. 2K+F22KF

4. BaCl2+H2SO4BaSO4+2HCl

Subtopic:  Introduction to Redox and Oxidation Number |
 65%
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Using the standard electrode potentials of the redox couples given below,
determine which of the following is the strongest oxidizing agent.

E values: Fe3+/Fe2+=+0.77
I2(s)/I-=+0.54;
Cu2+/Cu=+0.34; 
Ag+/Ag=0.80 V

1. Fe3+

2. I2(s)

3. Cu2+

4. Ag+

Subtopic:  Application of Electrode Potential |
 80%
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EΘ values of some redox couples are given below. On the basis of these values choose the correct option.

EΘ values: Br2/Br-=+1.90
Ag+/Ag(s)=+0.80
Cu2+/Cu(s)=+0.34; 
I2(s)/I-=+0.54

1. Cu will reduce Br- 2. Cu will reduce Ag
3. Cu will reduce I- 4. Cu will reduce Br2
Subtopic:  Emf & Electrode Potential |
 58%
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Using the standard electrode potential, find out the pair between which redox reaction is not feasible.

E values: Fe3+/Fe2+=+0.77; I2/I-=+0.54;
Cu2+/Cu=+0.34; Ag+/Ag=+0.80 V

1. Fe3+ and I-

2. Ag+ and Cu

3. Fe3+ and Cu

4. Ag and Fe3+

Subtopic:  Application of Electrode Potential |
 65%
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In the reactions given below, thiosulphate reacts differently with iodine than with bromine.

2S2O32-+I2S4O62-+2I-

S2O32-+2Br2+5H2O2SO42-+2Br-+10H+

Choose the statements among the following that best describe the above dual behaviour of thiosulphate.

1. Bromine is a stronger oxidant than iodine
2. Bromine is a weaker oxidant than iodine
3. Thiosulphate undergoes oxidation by bromine and reduction by iodine in these reactions
4. Bromine undergoes oxidation and iodine undergoes reduction in these reactions

Subtopic:  Oxidizing & Reducing Agents |
 61%
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The incorrect statement regarding the rule to find the oxidation number among the following is-

1. The oxidation number of hydrogen is always +1.
2. The algebraic sum of all the oxidation numbers carried by elements in a compound is zero.
3. An element in its free or uncombined state has an oxidation number of zero.
4. Generally, in all its compounds, the oxidation number of fluorine is -1.

Subtopic:  Oxidizing & Reducing Agents |
 77%
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In which of the following compounds, an element exhibits two different oxidation state?

1. NH2OH

2. NH4NO3

3. N2H4

4. N3H

Subtopic:  Oxidizing & Reducing Agents |
 83%
From NCERT
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