Water gas is an equimolar mixture of hydrogen and carbon monoxide. If 250L of water gas is burnt in air claculate the following assuming both reactants and products are at same temperature and pressure.

2CO + O₂ = 2CO₂; 2H₂ + O₂ = 2H₂O

1. Volume of carbon dioxide produced

a)125lb)62.5lc)250l d)500l

2. Volume of steam formed

a)62.5l b)250l c)125l d)375l

3. Volume of oxygen used up

a)250l b)125l c)75l d)500l

2CO + O₂ = 2CO₂; ---------1

2H₂ + O₂ = 2H₂O-----------2

Given CO + H₂  = 250 L

Since, CO and H₂ are equimolar, so each has vol 125L ( given total vol is 250L)

1. The equation shows that 

2 L vol of CO gives 2 L vol of CO₂ 

So, 125 L vol of CO gives 125 L vol of CO₂ 

Hence, option (a) is correct

2. The equation shows that 

2 L vol of  H₂ gives 2 L vol of H₂ O

So, 125 L vol of H₂ gives 125 L vol of H₂ O 

Hence, option (c) is correct

3. The equation 1 and 2 show that 

Half the volume of O₂ is used in both equation with respect to the CO and H₂ respectively, 

So, total volume of oxygen used is 125/2 L + 125/2 L = 125 L

Hence, option (b) is correct.