50 cm³ of carbon (II) oxide was exploded with 150 cm³ of air containing 20% oxygen by volume, which of the reactants was in excess?

 50 cm³ of carbon (II) oxide was exploded with 150 cm³ of air containing 20% oxygen by volume, which of the reactants was in excess?

A. Carbon (II) oxide

B. Carbon (IV) oxide

C. Oxygen

D. Nitrogen

First, write the balanced equation:

2CO + O_2 --> 2CO_2

 Step 1: Calculate the volume of oxygen in the air

Air contains 20% oxygen by volume.

Volume of  O_2 = 20/100 * 150 = 30 cm^3

 Step 2: Use the mole volume ratio

From the equation:

2 volumes of CO react with 1 volume of O₂

So:

30 cm³ of O₂ will react with

  2 * 30 = 60 cm^3  of CO

 Step 3: Compare with available volumes

Available CO = 50 cm³

Required CO = 60 cm³

Since less CO is available, carbon (II) oxide is the limiting reactant, and oxygen is in excess.

✅ Correct Answer: 

C. Oxygen

PQN: 36