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N₂H₄ + IO₃^- + 2H⁺ + Cl^- $\to$ICl + N₂ + 3H₂O
The equivalent masses of N₂H₄ and KIO₃ respectively are :-
1. 8 and 35.6
2. 8 and 87
3. 8 and 53.5
4. 16 and 53.5

What is the equivalent weight of H₃PO₃ in the following disproportionation reaction:-
H₃PO₃ $\to$H₃PO₄ + PH₃
1. $\frac{M}{6}$   
 2. $\frac{M}{2}$ 
3.  $\frac{2M}{3}$ 
 4. $\frac{M}{3}$

A brown ring complex compound is formulated as $\left[Fe{\left(H_{2}O\right)}_{5}NO\right]S{O}_4.$ The oxidation state of iron is 
1. 1
2. 2
3. 3
4. 0

Equivalent mass of FeS₂ in the half reaction, ${\mathrm{FeS}}_2\to {\mathrm{Fe}}_2{\mathrm{O}}_3+{\mathrm{SO}}_2$ is :
1. M/10
2. M/11
3. M/6
4. M/1

$6\times {10}^{-3}$ mole ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7$ reacts completely with $9\times {10}^{-3}$ mole ${\mathrm{X}}^{\mathrm{n}+}$ to give ${\mathrm{XO}}_3^{-}$ and ${\mathrm{Cr}}^{3+}$. The value of n is :
1. 1
2. 2
3. 3
4. None of these

1 mole of ${\mathrm{N}}_2{\mathrm{H}}_4$ loses 10 moles of electrons to form a new compound y. Assuming that all nitrogen appears in the new compound, what is the oxidation state of nitrogen in y?
(There is no change in the oxidation state of hydrogen)
1. +3
2. -3
3. -1
4. +5

The number of peroxide linkages in $K_{3}Cr{O}_8$ is/are 
1. 1
2. 2
3. 3
4. 4

A, B and C are three elements forming a part of compound in oxidation states of + 2 + 5 - 2 respectively. What could be the compound ?
1. $A_2{\left(BC\right)}_{2 }$
2.$A_2{\left(B{C}_4\right)}_3$
3.$A_3{\left(B{C}_4\right)}_{2 }$
4.$ABC$

Oxidation number of oxygen in potassium super oxide (KO₂) is:
1. – 2
2. – 1
3. – 1/2
4. – 1/4

If 1.2 g of metal displace 1.12 litre hydrogen at normal temperature and pressure, equivalent weight of metal would be 
(1) 24
(2) 12
(3) 1.2 $÷$ 11.2
(4) 1.2 $\times$ 11.2