<Dd> V 100 − V 0 = k V 0 (\ displaystyle V_ (100) - V_ (0) = kV_ (0) \,) </Dd> <P> where V is the volume occupied by a given sample of gas at 100 ° C; V is the volume occupied by the same sample of gas at 0 ° C; and k is a constant which is the same for all gases at constant pressure . This equation does not contain the temperature and so has nothing to do with what became known as Charles' Law . Gay - Lussac's value for k (​ ⁄), was identical to Dalton's earlier value for vapours and remarkably close to the present - day value of ​ ⁄ . Gay - Lussac gave credit for this equation to unpublished statements by his fellow Republican citizen J. Charles in 1787 . In the absence of a firm record, the gas law relating volume to temperature cannot be named after Charles . Dalton's measurements had much more scope regarding temperature than Gay - Lussac, not only measuring the volume at the fixed points of water, but also at two intermediate points . Unaware of the inaccuracies of mercury thermometers at the time, which were divided into equal portions between the fixed points, Dalton, after concluding in Essay II that in the case of vapours, "any elastic fluid expands nearly in a uniform manner into 1370 or 1380 parts by 180 degrees (Fahrenheit) of heat", was unable to confirm it for gases . </P> <P> Charles' law appears to imply that the volume of a gas will descend to zero at a certain temperature (− 266.66 ° C according to Gay - Lussac's figures) or − 273.15 ° C. Gay - Lussac was clear in his description that the law was not applicable at low temperatures: </P> <P> but I may mention that this last conclusion cannot be true except so long as the compressed vapours remain entirely in the elastic state; and this requires that their temperature shall be sufficiently elevated to enable them to resist the pressure which tends to make them assume the liquid state . </P>

What is the volume of a given mass of a gas at absolute zero temperature
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