The mole fraction of the solute in a 1.00 molal aqueous solution is: 

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

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

The hydrated salt, Na₂SO₄.nH₂O, undergoes a 55% loss in mass on heating and becomes anhydrous. The value of n will be:

The product of atomic mass and specific heat of 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

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:

2 gm Iron pyrite (FeS₂) is burnt with O₂ to form Fe₂O₃ and SO₂. The mass of SO₂ produced is (Fe=56, S=32, O=16)

1. 2 gm

2. 2.13 gm

3. 4 gm

4. 4.26 gm

Equivalent weight of ${\mathrm{FeS}}_2$ in the half reaction, ${\mathrm{FeS}}_2 \stackrel{}{\to } {\mathrm{Fe}}_2{\mathrm{O}}_3+{\mathrm{SO}}_2$ is:

1.  M/10

2.  M/11

3.  M/6

4.  M/1

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

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