Assertion (A):	In Haber's process, starting with 5 moles of N2 and 2.5 mol of H2, on complete reaction only 1.66 moles of  NH3 were produced.
Reason (R):	H2 acts as a limiting reagent in this reaction.

1.	Both (A) and (R) are true and (R) is the correct explanation of (A).
2.	Both (A) and (R) are true but (R) is not the correct explanation of (A).
3.	(A) is true but (R) is false.
4.	Both (A) and (R) are false.

 

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

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

 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 

1cc N₂O at STP contains: 

The number of valence electrons present in 0.53 grams of Na₂CO₃ is:

1. $3.01\times {10}^{23}$

2. $7.22\times {10}^{22}$

3. $12.046\times {10}^{23}$

4. $6.023\times {10}^{23}$