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4. An expandable container
that contains 500 L of argon
gas has an initial pressure of
1.00 atm. If the pressure was
increased to 4 058 mmHg,
calculate the final volume of
the container. Assume that the
temperature is constant.



Answer :

bharathparasad577

The final volume of the container that contains argon gas at 4058 mm of Hg is 93.80 L.

Given in the question

Initial pressure = 1.00 atm = P1

Initial volume = 500 L = V1

Final Pressure = 4058 mm of Hg = P2

To find

Final Volume = V2

Now, the unit of pressure is different for each case, So we need to convert mm of Hg into atmospheric pressure.

Using unitary method

760 mm of Hg = 1 atm

1 mm of Hg = 1/760 atm

1×4058 mm of Hg = 1/760 × 4058 atm

4.058 mm of Hg =  4058/760 atm

4.058 mm of Hg =  5.3 atm

Now as it is given in the question that the temperature remains constant, we can apply Boyle's law.

By using Boyle's law

P1V1 = P2V2

Put in the value

(1.0)(500) = (5.3)(V2)

V2 = 500/5.3

V2 = 93.80 L

Therefore, the final volume of the argon gas at 4058 mm of Hg is 93.80 L.

LEARN MORE ABOUT BOYLE'S LAW HERE: https://brainly.com/question/24938688

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