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

Answer: 2.0 fianal volume

Explanation:

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.