The oxidation number of carbon is correctly given for:
Compound  O.N.
(a) \(\mathrm{HN} \equiv \mathrm{C} \) +2
(b) \(\mathrm{H}-\mathrm{C}\equiv \mathrm{N} \) +4
(c) \(\mathrm{CCl}_4\) +4
(d) \(\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6 \) 0

1. a, b, c
2. b, c, d
3. a, c, d
4. None of the above
Subtopic:  Introduction to Redox and Oxidation Number |
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The oxidation state of two S-atoms in Na2S2O3 is:

1. +2 and +4

2. +3 and -2

3. +4 and -2

4. +6 and -2

Subtopic:  Introduction to Redox and Oxidation Number |
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What is the number of moles of electrons gained by one-mole oxidizing agent in the following redox reaction?

\( \mathrm{Zn}_{(s)} + \mathrm{2HCl}_{(aq)} \rightarrow \mathrm{ZnCl_2}_{(aq)}+\mathrm {H_2} _{(g)}\)

1. 4
2. 3
3. 2
4. 1
Subtopic:  Introduction to Redox and Oxidation Number |
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Oxidation number of oxygen is minimum in
1. Oxides
2. Peroxides
3. Superoxides
4. Dioxygen
Subtopic:  Introduction to Redox and Oxidation Number |
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The oxidation states of \(\text {Cr}\) in \(\left[\mathrm{Cr}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right] \mathrm{Cl}_3\),\( \left[\mathrm{Cr}\left(\mathrm{C}_6 \mathrm{H}_6\right)_2\right] \) and \(\mathrm{K}_2\left[\mathrm{Cr}(\mathrm{CN})_2(\mathrm{O})_2\left(\mathrm{O}_2\right)\left(\mathrm{NH}_3\right)\right]\) respectively are:

1. +3, +4, and +6 
2. +3, +2, and +4
3. +3, 0, and +6 
4. +3, 0, and +4
Subtopic:  Introduction to Redox and Oxidation Number |
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In the given reaction, the oxidation state of Cl in the major product will be:

\(\mathrm{Cl}_2 \mathrm{O}_7+\mathrm{H}_2 \mathrm{O}_{2} \rightarrow \)

1. +1
2. +2
3. +3
4. +5
Subtopic:  Introduction to Redox and Oxidation Number |
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In the following reaction, \(X, Y\) and \(Z\) are respectively:
 \(XZn+ NO^- _3+ YH^+ \rightarrow XZn^{2+}+ NH^+ _4+ ZH_2O \)

1. 4, 10, 3 
2. 3, 8, 3
3. 3, 10, 3
4. 4, 3, 10
Subtopic:  Balancing of Equations |
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The oxidation number of Cr in \(K_3CrO_8\) will be:
 
1. +13 
2. +7 
3. +6 
4. +5
Subtopic:  Introduction to Redox and Oxidation Number |
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Balance the following half-reaction in acidic solution:
\(\text{NO}^-_3\rightarrow \text{NH}^+_4\) 
When balanced with the smallest whole-number coefficients, what is the sum of all the coefficients and electrons used?
1. 13
2. 26
3. 15
4. 23
Subtopic:  Balancing of Equations |
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Consider the given reaction:
\(\mathrm{Al}+\mathrm{Fe}_3 \mathrm{O}_4 \rightarrow \mathrm{Al}_2 \mathrm{O}_3+\mathrm{Fe}\)

What is the total number of electrons transferred in the given reaction?
1. 6
2. 8
3. 8/3
4. 24

Subtopic:  Balancing of Equations |
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