Question

200 ml of hydrogen in 250 ml of Nitrogen each measure at 15 degrees centigrade and 760 mm pressure at together in 500 ml flask what will be the final pressure of the mixture at 15 degree celsius ​

Answer 1

If 200 ml of H2 & 250 ml of N2 at 760 mmHg are kept in 500 ml flask together then the final pressure of the mixture at 15-degree Celsius is 684 mmHg.

Explanation:

Here the temperature for both the cases is given to be constant.

For Hydrogen:

Initial pressure, P₁ = 760 mmHg  

Initial volume, V₁ = 200 ml  

Final volume, V₂ = 500 ml

Final pressure in the mixture, P₂ = ?

Using Boyle’s Law, we have

P₁V₁ = P₂V₂

⇒ 760 * 200 = P₂ * 500

⇒ P₂ = [760 * 2] / 5

⇒ P₂ = 304 mmHg ← Final pressure of H2 in the mixture

For Nitrogen:

Initial pressure, P₁ = 760 mmHg  

Initial volume, V₁ = 250 ml  

Final volume, V₂ = 500 ml

Final pressure in the mixture, P₂ = ?

Using Boyle’s Law, we have

P₁V₁ = P₂V₂

⇒ 760 * 250 = P2 * 500

⇒ P2 = [760 * 250] / 500

⇒ P2 = 380 mmHg ← Final pressure of N2 in the mixture

Thus,  

The final of the mixture of H2 & N2 at 15℃ is,

= [Final pressure of H2 in the mixture] + [Final pressure of N2 in the mixture]

= [308 + 380] mmHg

= 684 mmHg

Learn more from the below links:

Example problem of boyle's law with solution

https://brainly.ph/question/541714

Numericals based on Boyle's law

https://brainly.in/question/1877258