. Stoichiometry . 0125 -0 125 0 250 0 375. 3375 6750 10125 13 500 20 250 e Fig. 55.—Diagrams of the deviations from the laws relating to perfect gaseswhich would be observed in the case of gases under low pressures if theformula of Van der Waals were applicable to i.—Deviation from Boyles 2.— ,, ,, Avogadros (Amperes) law. Diagram 3.— „ „ Gay Lussacs law. Diagram 4.—Thermal effects produced during expansion. Curve Tg.—Thermal effect due to external work, resulting from variation in value of Ti.—Thermal effect due to internal T;.—Joule-Thomson effect
. Stoichiometry . 0125 -0 125 0 250 0 375. 3375 6750 10125 13 500 20 250 e Fig. 55.—Diagrams of the deviations from the laws relating to perfect gaseswhich would be observed in the case of gases under low pressures if theformula of Van der Waals were applicable to i.—Deviation from Boyles 2.— ,, ,, Avogadros (Amperes) law. Diagram 3.— „ „ Gay Lussacs law. Diagram 4.—Thermal effects produced during expansion. Curve Tg.—Thermal effect due to external work, resulting from variation in value of Ti.—Thermal effect due to internal T;.—Joule-Thomson effect. 2icS sTO/c7/n)j//:7/xv is correct, but Berthelot has collected all the available data for hydro-gen, nitrogen, carbon monoxide, air, oxygen, nitric oxide, methane, and carbon dioxide, and calculated the values of V, ^ from them. air These values, plotted against t, fall satisfactorily on a parabola,which, however, is quite distinct from that derived from Clausiusequation. Moreover, the limiting value is not J, but |,
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