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Percentage of Se in peroxidase anhydrase enzyme is 0.5% by weight (at. weight = 78.4), then minimum molecular weight of peroxidase anhydrase enzyme is
1. 1.568 x 10³ 
2. 15.68
3. 2.168 x 10⁴ 
4. 1.568 x 10⁴ 

Number of moles of Mn${\mathrm{O}}_4^{-}$ required to oxidise one mole of ferrous oxalate completely in acidic medium will be 
1. 0.6 mole
2. 0.4 mole
3. 7.5 moles
4. 0.2 mole

The total number of valence electrons in 4.2g of ${\mathrm{N}}_3^{-}$ ion is (N_A is the Avogadro's number)
1. 2.1N_A 
2. 4.2N_A 
3. 1.6N_A 
4. 3.2N_A 

The mass of carbon anode consumed (giving only carbon dioxide) in the production of 270 kg of aluminium metal from bauxite by the Hall process is (at. mass of Al = 27)
1. 180 kg
2. 270 kg
3. 540 kg
4. 90 kg

A metal oxide has the formula Z₂O_3. It can be reduced by hydrogen to give free metal and water. 0.1596g of the metal oxide requires 6 mg of hydrogen for complete reduction. The atomic weight of the metal is
1. 27.9
2. 159.6
3. 79.8
4. 55.8

In the Haber process, 30 L of dihydrogen and 30 L of dinitrogen were taken for the reaction, which yielded only 50% of the expected product. The composition of the gaseous mixture under the said conditions at the end is: 
1. 20 L ammonia, 10 L nitrogen, 30 L hydrogen
2. 20 L ammonia, 25 L nitrogen, 15 L hydrogen
3. 20 L ammonia, 20 L nitrogen, 20 L hydrogen
4. 10 L ammonia, 25 L nitrogen, 15 L hydrogen

A partially dried clay mineral contains 8% water. The original sample contained 12% water and 45% silica. The percentage of silica  in the partially dried sample is nearly:

One mole of a mixture of CO and CO₂ requires exactly 20g of NaOH in solution for the complete conversion of all the CO₂ into Na₂CO₃. How much NaOH would it require for conversion into Na₂CO₃, if the mixture (one mole) is completely oxidised to CO₂?
1. 60g
2. 80g
3. 40g
4. 20g

When 100 mL of PH₃ is decomposed, it produces phosphorus and hydrogen. The change in volume is:

Mass of sucrose C₁₂H₂₂O₁₁ produced by mixing 84 gm of carbon, 12gm of hydrogen and 56L. O₂ at 1atm & 273 K according to give reaction, is C(s) + H₂(g) +O₂(g) $\to$ C₁₂H₂₂O₁₁ (s)
1. 138.5
2. 155.5
3. 172.5
4. 199.4

1.0 mol of Fe reacts completely with 0.65 mol of O₂ to give a mixture of only FeO and Fe₂O₃. The mole ratio of ferrous oxide to ferric oxide is
(1) 2 : 2
(2) 4 : 3
(3) 1 : 2
(4) 2 : 7

KClO₃ on heating decomposes to KCl and O₂. The volume of O₂ at STP liberated by 0.1 mole KClO₃ is
1. 4.36 L
2. 3.36 L
3. 2.36 L
4. None of these

Total number of moles of oxygen atoms in 3 litre ${\mathrm{O}}_3\left(\mathrm{g}\right)$ at 27$°$C and 8.21 atm are:
1.  3
2.  1
3.  2
4.  none of these

The equivalent weight of $\mathrm{HCl}$ in the given reaction is: ${\mathrm{K}}_2{\mathrm{Cr}}_2{\mathrm{O}}_7+14\mathrm{HCl} \to 2\mathrm{KCl}+2{\mathrm{CrCl}}_3+3{\mathrm{Cl}}_2+{\mathrm{H}}_2\mathrm{O}$
1.  16.25
2.  36.5
3.  73
4.  85.1

Cisplatin, an anticancer drug, has the molecular formula $\mathrm{Pt}{\left({\mathrm{NH}}_3\right)}_2 {\mathrm{Cl}}_2$. What is the mass (in gram) of one molecule? (Atomic weights : Pt=195, H=1.0, N=14, Cl=35.5)
1.  $4.98\times {10}^{-21}$
2.  $4.98\times {10}^{-22}$
3.  $6.55\times {10}^{-21}$
4.  $3.85\times {10}^{-22}$

A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. It's density is 2.28 g/litre at 300 K and 1.0 atm pressure. Determine the molecular formula of the compound:
1.  ${\mathrm{C}}_2{\mathrm{H}}_2$
2.  ${\mathrm{C}}_2{\mathrm{H}}_4$
3.  ${\mathrm{C}}_4{\mathrm{H}}_8$
4.  ${\mathrm{C}}_4{\mathrm{H}}_{10}$

Copper forms two oxides. For the same amount of copper, twice as much oxygen was used to form first oxide than to form second one. What is the ratio of the valencies of copper in first and second oxides?
1. 2:5
2. 1:6
3. 2:1
4. 1:2

The average molar mass of the mixture of ${\mathrm{CH}}_4$ $$and ${\mathrm{C}}_2{\mathrm{H}}_4$ present in the mole ratio of a:b is
20 g mol^-1. When the mole ratio is reversed, the molar mass of the mixture will be:

The vapour density of a volatile chloride of a metal is 95 and the specific heat of the metal is 0.13 cal/g. The equivalent mass of the metal will be:
1.  6 g
2. 12 g
3.  18 g
4.  24 g

Equivalent weight of ${\mathrm{H}}_3{\mathrm{PO}}_2$ when it disproportionate into ${\mathrm{PH}}_3$ and ${\mathrm{H}}_3{\mathrm{PO}}_3$ is:
1. M
2. M/2
3. M/4
4. 3M/4

The angular momentum of an electron in d orbital is equal to
1. $\sqrt{6} \sout{\mathrm{h}}$
2. $\sqrt{2} \mathrm{h}$
3. $2\sqrt{3} \mathrm{h}$
4. 0 h