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$The number of KMn{O}_{4 }reduced by one mole of KI in alkaline medium is$
1. One fifth
2. five
3. one
4. two

The hydrated salt ${\mathrm{Na}}_2{\mathrm{SO}}_4.{\mathrm{nH}}_2\mathrm{O},$ undergoes 55% loos in mass on heating and becomes anhydrous. The value of n will be:
1.  5
2.  3
3.  7
4.  10

Assuming fully decomposed, the volume of $C{O}_2$ released at STP on heating 9.85g of $BaC{O}_3$(At  mass of Ba=137) will be 
1. 1.12L
2. 0.84L
3. 2.24L
4. 4.96L

The molality of 15% (w/vol.) solution of ${\mathrm{H}}_2{\mathrm{SO}}_4$ of density 1.1 g/cm³ is approximately:
1.  1.2
2.  1.4
3.  1.8
4.  1.6

200Kg of iron ore $\left(F{e}_2{O}_3\right)$ containing 20% impurities, on reduction with CO give iron. The Amount of iron produced will be-
1. 84kg
2. 200kg
3. 56kg
4. 112kg

The product of atomic mass and specific heat of a metal is approximately 6.4. This was given by:
1.  Dalton's law
2.  Avogadro's law
3.  Newton's law
4.  Dulong Petit's law

The chloride of a metal contains 71% chlorine by mass and the vapour density of it is 50. The atomic mass of the metal will be:
1.  29
2.  58
3.  35.5
4.  71

100 mL of ${\mathrm{PH}}_3$ when decomposed produces phosphorus and hydrogen. The change in volume is:
1.  50 mL increase
2.  500 mL decrease
3.  900 mL decrease
4.  none of these

When a solution containing 4.77 gm of NaCl is added to a solution of 5.77 gm of  AgNO₃. The weight of precipitated AgCl is:
1. 11.70 gm
2. 9.70 gm
3. 4.86 gm
4. 2.86 gm

0.4g of a polybasic acid $H_{n}A$(all the hydrogens are acidic ) requires 0.5g of NaOH for complete neutralization. The number of replaceable hydrogen atoms in the acid and the molecular weight of 'A' would be:(Molecular Weight of the acid is 96 gms.).
1. 1,95
2. 2,94
3. 3,93
4, 4,92

The number of moles of oxygen in 1L of air containing 21% oxygen by volume, under standard conditions, is
1.  0.0093 mole
2.  2.10 mole
3.  0.186 mole
4.  0.21 mole

A sample of pure compound is found to have Na= 0.0887 mole, O= 0.132 mole, C= $2.65\times {10}^{22}$atoms. The empirical formula of the compound is
1. $N{a}_{2}C{O}_3$
2. $N{a}_3{O}_2{C}_5$
3. $N{a}_{0.0887}{O}_{0.132}{C}_{2.65\times {10}^{22}}$
4. NaCO

Suppose the elements X and Y combine to form two compounds XY₂ and X₃Y₂. When 0.1 mole of XY₂ weighs 10 g and 0.05 mole of X₃Y₂ weights 9 g, the atomic weights of X and Y are
1.  40, 30
2.  60, 40
3.  20, 30
4.  30, 20

If 10 gm of ${\mathrm{V}}_2{\mathrm{O}}_5$ is dissolved in acid and is reduced to ${\mathrm{V}}^{2+}$ by zinc metal, how many mole of ${\mathrm{I}}_2$ could be reduced by the resulting solution if it is further oxidised to ${\mathrm{VO}}^{2+}$ ions? [Assume no change in state of ${\mathrm{Zn}}^{2+}$ ions] (V=51, O=16, I=127):
1.  0.11 mole of ${\mathrm{I}}_2$
2.  0.22 mole of ${\mathrm{I}}_2$
3.  0.005 mole of ${\mathrm{I}}_2$
4.  0.44 mole of ${\mathrm{I}}_2$

The mass of carbon present in 0.5 mole of $K_4\left[Fe\right(CN{)}_6]$ is
1. 1.8 g
2. 18 g
3. 3.6 g
4. 36 g

Concentrated aqueous sulphuric acid is 98% ${\mathrm{H}}_2{\mathrm{SO}}_4$ by mass and has a density of 1.80 g mL^-1. Volume of acid required to make one litre of 0.1 M ${\mathrm{H}}_2{\mathrm{SO}}_4$ solution is:
1.  11.10 mL
2.  16.65 mL
3.  22.20 mL
4.  5.55 mL

The total number of electrons present in 1.6 gm of methane is
1. $6\times {10}^{23}$
2. $6.02\times {10}^{22}$
3. $6.02\times {10}^{21}$
4. $4.02\times {10}^{20}$

A mixed solution of potassium hydroxide and sodium carbonate required 15ml of an N/20 
HCl solution when titrated with phenolphthalein as an indicator. But the same amount of the solution when titrated with methyl orange as an indicator required 25ml of the same acid. The amount of KOH present in the solution 
1. 0.014g
2. 0.14g
3. 0.028g
4. 1.4g

Oxygen contains 90% $O^{16 }$ and 10% $O^{18}$. Its atomic mass is
1. 17.4
2. 16.2
3. 16.5
4. 17