If a gas occupies a volume of 0.25 L at –2.3°C, by what amount would the volume increase if the gas were heated to 82°C at constant pressure?

Could somebody include the whole process? I'm really confused

This in accordance with Boyle's law which states that the product of the initial pressure and volume is equal to the product of the final pressure and volume.

P1V1 = P2V2

Now compare this to Charles ' law which states that the product of the initial volume and the final temperature is equal to the product of the final volume and initial temperature.

V1T2= V2T1

Remember that all temperatures must be calculated in kelvin

If the initial temperature of 273 K is doubled to 546 K,

then a initial volume of 1.0 liter is also doubled, with a final volume of 2.0 liters.

If a gas occupies a volume of 0.25 L at –2.3°C, by what amount would the volume increase if the gas were heated to 82°C at constant pressure? Could somebody include the whole process? I'm really confused

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If a gas occupies a volume of 0.25 L at –2.3°C, by what amount would the volume increase if the gas were heated to 82°C at constant pressure?

Could somebody include the whole process? I'm really confused