Question

This is the equation for the combustion of carbon monoxide is: CO + O2

CO2
How many liters of oxygen are needed to burn 2.76 L of carbon monoxide?

Answer 1

Answer: 1.38 L O2

Step-by-step explanation:

2CO + O2 = 2CO2

So,

1 mole CO = 22.4 L CO

2 mole CO = (22.4 ×‌‍‍2)L CO

= 44.8 L CO

And 1 mole O2 = 22.4 L O2

44.8LCO are burned by 22.4LO2 1 L CO are burned by 22.4÷ 44.8

= 0.5 L O2

2.76L CO are burned by0.5×2.76

= 1.38 L O2

So, 1.38 L O2 are needed to burn

2.76 L CO

Answer 2

Answer: 1,38 litres

Explanation: it should be 2 CO + O2 ⇒ 2 CO2

In Same temperature volumes are proportional

To amounts of substances. So amount of Oxygen is half of

Amount of CO