In Haber process 30L of  dihydrogen and 30L of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gasesous mixture under the a fore said condition in the end?

(a) 20L ammonia, 10L nitrogen, 30L hydrogen

(b) 20L ammonia, 25L nitrogen, 15L hydrogen

(c) 20L ammonia, 20L nitrogen, 20L hydrogen

(d) 10L ammonia, 25L nitrogen, 15L hydrogen

1 gm butane (C₄H₁₀) is burnt with excess of O₂ to form CO₂. The approximate mass of CO₂ produced is

1. 1gm

2. 2gm

3. 3gm

4. 4gm

0.5 mole of BaCl₂ is reacted with 0.2 mole Na₃PO₄ then maximum moles of Ba₃(PO₄)₂ formed is 

1. 0.33

2. 0.2

3. 0.1

4. 0.5

25.4 of ${\mathrm{I}}_2$ and 14.2 g  of ${\mathrm{Cl}}_2$ are made to react completely to yield a mixture of ICI and ICI₃. Calculate mole of ICI and ICI₃ formed.

1. 0.5 ,02

2.0.1, 0.1

3. 0.1 ,0.3

4. 0.3,0.4

60 mL of a mixture of nitrous oxide and nitric oxide was exploded with excess of hydrogen. If 38 mL of ${\mathrm{N}}_2$ was formed, calculate the volume of each gas in the mixture. All measurements are made at constant P and T.

1.20 ml +30 ml

2. 44 ml + 16 ml

3. 10 ml+40 ml

4 .25 ml +25 ml