According to Charles' Law, if a gas occupies 22.4 L at 0°C, what volume does it occupy at 273°C, assuming ideal gas behavior?

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Multiple Choice

According to Charles' Law, if a gas occupies 22.4 L at 0°C, what volume does it occupy at 273°C, assuming ideal gas behavior?

Explanation:
Volume is proportional to absolute temperature when pressure and amount of gas stay the same. That means using Kelvin temperatures to compare volumes: V2 = V1 × (T2/T1). Convert temperatures to Kelvin: 0°C is 273.15 K, and 273°C is 546.15 K. The temperature ratio is 546.15 / 273.15 ≈ 2.00. With V1 = 22.4 L, the new volume is 22.4 L × 2.00 ≈ 44.8 L. So the gas expands to about 44.8 liters at 273°C under constant pressure.

Volume is proportional to absolute temperature when pressure and amount of gas stay the same. That means using Kelvin temperatures to compare volumes: V2 = V1 × (T2/T1).

Convert temperatures to Kelvin: 0°C is 273.15 K, and 273°C is 546.15 K. The temperature ratio is 546.15 / 273.15 ≈ 2.00. With V1 = 22.4 L, the new volume is 22.4 L × 2.00 ≈ 44.8 L.

So the gas expands to about 44.8 liters at 273°C under constant pressure.

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