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lozanna [386]
2 years ago
14

A sample of oxygen that occupies 1.00 * 10^6 at 575 mm Hg is subjected to a pressure of 1.25 atm. What will the final volume of

the sample be if the temperature is held constant?
Chemistry
1 answer:
Vlada [557]2 years ago
5 0

A sample of oxygen occupies 1.00 × 10⁶ mL at 575 mmHg. If the pressure is increased to 1.25 atm, the volume decreases to 6.06 × 10⁵ mL.

<h3>What does Boyle's law state?</h3>

Boyle's law states that the pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature.

  • Step 1: Convert the initial pressure to atm.

We will use the conversion factor 1 atm = 760 mmHg.

575 mmHg × 1 atm/760 mmHg = 0.757 atm

  • Step 2: Calculate the final volume of the gas

A sample of oxygen occupies 1.00 × 10⁶ mL (V₁) at 0.757 atm (P₁).

If the pressure is increased to 1.25 atm (P₂), we can calculate the new volume (V₂) using Boyle's law.

P₁ × V₁ = P₂ × V₂

V₂ = P₁ × V₁ / P₂

V₂ = 0.757 atm × 1.00 × 10⁶ mL / 1.25 atm = 6.06 × 10⁵ mL

A sample of oxygen occupies 1.00 × 10⁶ mL at 575 mmHg. If the pressure is increased to 1.25 atm, the volume decreases to 6.06 × 10⁵ mL.

Learn more about Boyle's law here: brainly.com/question/469270

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