The mass of carbon present in 0.5 mole of K₄[Fe(CN)₆] is:

1.	1.8 g	2.	18 g
3.	3.6 g	4.	36 g

ln, a closed vessel, 50 ml of $A_2{B}_3$ completely reacts with 200 ml of C₂ according to the following equation:

$2A_2{B}_3\left(g\right) + 5C_2\left(g\right)\to 3C_3{B}_2\left(g\right)+C{A}_4\left(g\right)$

The composition of the gaseous mixture in the system will be:

1. 100 ml $C_2, 50 ml C_3{B}_2,50 ml C{A}_4$

2. 25 ml $C_2, 75 ml C_3{B}_{\mathrm{2,}} 25 ml C{A}_4$

3. 75 ml $C_2, 75 ml C_3{B}_{2, }25 ml C{A}_4$

4. 10 ml $C_2, 25 ml C_3{B}_{2, }100 ml C{A}_4$

The density of a 2 M aqueous solution of NaOH is 1.28 g/$c{m}^3$. The molality of the solution is: 
[molecular mass of NaOH = 40 $gmo{l}^{-1}$]

On complete combustion, 44 g of a sample of a compound gives 88 g CO₂ and 36 g of H₂O. The molecular formula of the compound may be:

1.  ${\mathrm{C}}_4{\mathrm{H}}_6$ $$

2.  ${\mathrm{C}}_2{\mathrm{H}}_6\mathrm{O}$ $$

3.  ${\mathrm{C}}_2{\mathrm{H}}_4\mathrm{O}$

3.  ${\mathrm{C}}_3{\mathrm{H}}_6\mathrm{O}$

The molality of pure water is: 

1. 1 m

2. 18 m

3. 55.5 m

4. None of the above

 The maximum number of molecules is present in which of the following? 

1. 15 L of $H_2$ gas at STP

2. 5 L of $N_2$ gas at STP

3. 0.5 g of $H_2$ gas

4. 10 g of $O_2$ gas

The number of  moles  present in 2.5 litres of 0.2 M  ${\mathrm{H}}_2{\mathrm{SO}}_4$ are:

1. 0.25

2. 0.5

3. 0.75

4. 0.2

Which of the following statements is correct?

1. 1 mole of electrons weights 5.4 mg 
2. 1 mole of electrons weights 5.4 kg 
3. 1 mole of electrons weights 0.54 mg 
4. 1 mole of electrons has 1.6$\times {10}^{-19}$ C of charge