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    When investigating Boyle's Law P proportional to 1/V. It is advised to change the pressure (e.g. using a foot pump) slowly in order that temperature is not affected.

    I understand that temperature is related to temeprature by the ideal gas equation: pV = nRT however, why would a slow increase in pressure not affect the temperature opposed to a fast increase. Or is it that any increase in the thermal energy can be quickly transferred to the surroundings so it is negligible if you slowly increase the pressure?
    Regards, Adam
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    (Original post by splitter2017)
    When investigating Boyle's Law P proportional to 1/V. It is advised to change the pressure (e.g. using a foot pump) slowly in order that temperature is not affected.

    I understand that temperature is related to temeprature by the ideal gas equation: pV = nRT however, why would a slow increase in pressure not affect the temperature opposed to a fast increase. Or is it that any increase in the thermal energy can be quickly transferred to the surroundings so it is negligible if you slowly increase the pressure?
    Regards, Adam
    My guess would be that your reducing the volume to increase pressure making it so that overall your value for 'PV' remains the same and hence 'nRT' stay the same also. This would mean temperature would remain constant.

    But then again, this is just an educated guess Hope this helped anyways :P
 
 
 
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