Question

a sample of Oxygen gas occupies a volume of 250 ml at 740 mm HG pressure what volume will it occupy at 800 Torr pressure​

Answer 1

Explanation:

• P1V1=P2P2
• 740torr*250ml=800torr*V2
• 231.25ml

Answer 2

Answer:

The final volume of the sample of oxygen gas, V₂, calculated is $231.25ml$.

Explanation:

Given data,

The initial volume of the sample of oxygen gas, V₁ = $250ml$

The initial pressure of the sample of oxygen gas, P₁ = $740mmHg$

The final pressure of the sample of oxygen gas, P₂ = $800torr$

The final volume of the sample of oxygen gas, V₂ =?

Firstly, we have to convert the initial pressure unit into the torr.

• $1mmHg$ = $1torr$

So,

• $740mmHg$ = $740torr$

Now, by using Boyle's law, we can find out the final volume of the sample of oxygen gas:

• $P_{1} V_{1} = P_{2} V_{2}$

After substituting the value of the given pressures and volume in the above-mentioned formula, we get:

• $740\times 250 = 800\times V_{2}$
• V₂ = $\frac{185000}{800}$
• V₂ = $231.25$ml

Hence, the final volume of the sample of oxygen gas, V₂, calculated is $231.25ml$.