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    Gay-Lussacs Law is an where at constant volume the pressure of an ideal gas is directly proportional to its absolute temperature. In other words Gay-Lussac’s Law states that the pressure of a fixed amount of gas at fixed volume is directly proportional to its temperature in kelvins.
    Simplified this means that if you increase the temperature of a gas the pressure rises proportionally. Pressure and temperature will both increase or decrease simultaneously as long as the volume is held constant.
    The law has a simple mathematical form if the temperature is measured on an absolute scale such as in kelvins. The Gay-Lussacs Law is expressed as:
    ##(P_1)/(T_1)## = ##(P_2)/(T_2)##
    Where ##P_1## stands for the initial pressure of the gas ##T_1## stands for the initial temperature ##P_2## stands for the final pressure of the gas and ##T_2## stands for the final temperature.
    This law holds true because temperature is a measure of the average kinetic energy of a substance; when the kinetic energy of a gas increases its particles collide with the container walls more rapidly and exert more pressure.
    Take a sample of gas at STP 1 atm and 273 K and double the temperature.
    ##(1 atm)/(273 K) = P/(546 K)##
    ##(546 atm K)/(273 K) = P##
    P = 2 atm
    Doubling the temperature likewise doubled the pressure.

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