If 500 cm³ of gas, having a pressure of 760 millimeters of mercury, is compressed into a volume of 300 cm³ given the temperature remains constant, the pressure of the gas will be, in millimeters of mercury, approximately:
Correct answer: D. 1,270 mm of Hg
- A. 500 mm of Hg
- B. 900 mm of Hg
- C. 1,100 mm of Hg
- D. 1,270 mm of Hg
Explanation
Since the temperature is constant, this follows Boyle's Law: P₁V₁ = P₂V₂. We have P₁ = 760 mmHg, V₁ = 500 cm³, and V₂ = 300 cm³. Solving for the final pressure, P₂ = (P₁V₁) / V₂ = (760 × 500) / 300 ≈ 1267 mmHg, which is closest to 1,270.
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About Boyle's Law
Boyle's law states that the pressure of a fixed mass of gas varies inversely with its volume when temperature remains constant. Problems use the relationship P₁V₁ = P₂V₂, pressure-volume graphs and volume changes, with constant temperature distinguishing it from Charles's law.
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