Oxidation state of nitrogen is incorrectly given for:      

Compound	Oxidation state
1. (Co(NH3)5Cl)Cl2	-3
2. NH2OH	-1
3. (N2H5)2SO4	+2
4. Mg3N2	-3

A, B and C are three elements forming a part of
compound in oxidation states of +2, +5 and –2
respectively. What could be the compounds?

1. ${\mathrm{A}}_2{\left(\mathrm{BC}\right)}_2$

2. ${\mathrm{A}}_2{\left({\mathrm{BC}}_4\right)}_3$

3. ${\mathrm{A}}_3{\left({\mathrm{BC}}_4\right)}_2$

4. ABC

Consider the following reaction :

${\mathrm{xMnO}}_4^{-} + {\mathrm{yC}}_2{\mathrm{O}}_4^{2-} + {\mathrm{zH}}^{+} \to {\mathrm{xMn}}^{2+} +\hspace{0.17em}2{\mathrm{yCO}}_2 +\hspace{0.17em}\frac{\mathrm{z}}{2}{\mathrm{H}}_2\mathrm{O}$

The values of x, y and z in the reaction are
respectively :

1. 2, 5 and 16

2. 5, 2 and 8

3. 5, 2 and 16

4. 2, 5 and 8

Valency factor $\left({\mathrm{V}}_t\right)$ for following redox reaction is respectively.

a. ${\mathrm{As}}_2{\mathrm{S}}_3 \to {\mathrm{AsO}}_4^{-3}+{\mathrm{SO}}_4^{2-}$

b. ${\mathrm{I}}_2 \to {\mathrm{I}}^{-}+{\mathrm{IO}}_3^{-}$

c. ${\mathrm{H}}_3{\mathrm{PO}}_2 \to {\mathrm{PH}}_3+{\mathrm{H}}_3{\mathrm{PO}}_3$

1. $28, \frac{5}{3},\frac{4}{3}$

2. $28,\frac{4}{3},\frac{5}{3}$

3. $6, 4, 7$

4. 4, 3, 9

The oxidation number of phosphorus in Ba(H₂PO₂)₂ is:

1. +3

2. +2

3. +1

4. -1

The oxidation state of Cr in [Cr(NH₃)₄Cl₂]⁺ is:

1. +3

2. +2

3. +1

4. 0

A redox reaction among the following is

1. $CdC{l}_2+2KOH\to Cd{\left(OH\right)}_2+2KCl$

2. $BaC{l}_2+K_{2}S{O}_4\to BaS{O}_4+2KCl$

3. $CaC{O}_3\to CaO+C{O}_2$

4. $2Ca+O_2\to 2CaO$

The reducing ability of the metals K, Au, Zn, and Pb follows the order

Which of the following transformations can be carried out by using HI as a reducing agent, under acidic conditions? $[Given: I_2(s)\to 2I^{-} E°=0.54 V]$

(i) $C{u}^{+}\to Cu\left(s\right) E°=0.52 V$

(ii) $C{r}^{3+}\to C{r}^{2+} E°=-0.41$

(iii) $F{e}^{3+}\to F{e}^{2+} E°=0.77 V$

(iv) $F{e}^{2+}\to Fe\left(s\right) E°=-0.44 V$

1. (i) and (iii)

2. (ii) and (iv)

3. only (iii)

4. Only (ii)

A solution (5 mL) of an acid X is completely neutralised by y mL of 1 M NaOH. The same volume (y mL) of 1 M NaOH is required to neutralise 10 mL of 0.6 M of $H_{2}S{O}_4$ completely. The normality (N) of the acid X is

1. 1.2

2. 2.4

3. 4.8

4. 0.6