Gay-Lussac's Law states that the ratio of absolute pressure to the absolute temperature remains constant for a fixed volume and a fixed mass or moles of an Ideal Gas. The Ideal Gas Law gives:
PV = nRT
P/T = nR/V = kGL
The constant in Gay-Lussac's Law depends upon the moles of gas and volume occupied by that gas
and is given by :
kGL = nR/V
where
n = moles of gas
R = universal gas constant
V = volume.
For one mole of Ideal Gas at occupying 22.4 liters, the constant ( kGL ) would be :
kGL = ( n )( R ) / ( V )
kGL = ( 1.0 gmol ) ( 0.08206 atm - L / gmol -K ) / ( 22.4 L )
kGL = 0.003663 atm / K .
ANSWER: kGL = nR/V
k is the ratio P/T at constant volume.
If any other units are used, the value will be different. --Depending on the units you chose the value of the constant differs
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V/T = constant
The Gas Law, PV=nRT.
The pressure must be maintained constant.
If any other units are used, the value will be different. --Depending on the units you chose the value of the constant differs
how does the rate law show how concentration changes after the rate of reaction
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The constant k is a...constant specific for the system considered.
This is the Boyle law (or Boyle-Mariotte law).
Boyles Law deals with conditions of constant temperature. Charles' Law deals with conditions of constant pressure. From the ideal gas law of PV = nRT, when temperature is constant (Boyles Law), this can be rearranged to P1V1 = P2V2 (assuming constant number of moles of gas). When pressure is constant, it can be rearranged to V1/T1 = V2/T2 (assuming constant number of moles of gas).