Question

what is the volume of phosgene which is formed at STP when 11.2 litres of chlorine reacts with carbon monoxide?​

Answer 1

Answer:

11.2 L

Explanation:

The reaction is CO+Cl 2 ​ → COCl 2 ​ . One mole of CO gives one mole of phosgene.

At STP, one mole of any gas occupies 22.4 L. 22.4 L of CO will give 22.4 L of phosgene at STP.

Thus, 11.2 L of CO will give 11.2 L of phosgene.

Answer 2

Answer:

At STP, the volume of phosgene formed is $11.2L$.

Explanation:

Given,

At STP, the volume of chlorine gas = $11.2L$

At STP, the volume of phosgene formed =?

Here, STP is standard temperature and pressure.

Now,

• The reaction of carbon monoxide with chlorine occurs in the way given below:
• $CO + Cl_{2} \rightarrow COCl_{2}$

From this reaction, we can say that one mole of chlorine gas gives 1 mole of phosgene.

• Number of moles of chlorine gas = Number of moles of phosgene

As we know,

• At STP, one mole of any gas occupies $22.4L$.

Now,

• Number of moles of gas at STP = $\frac{Volume of gas at STP}{22.4L}$ = $\frac{11.2}{22.4}$ = $0.5mol$

Thus,

• The volume of phosgene at STP = number of moles × $22.4 L$
• The volume of phosgene at STP = $0.5 \times 22.4$ = $11.2L$.