This historic book may have numerous typos and missing text. Purchasers can download a free scanned copy of the original book (without typos) from the publisher. Not indexed. Not illustrated. 1920 Excerpt: ...is the empirical formula obtained by him and g subsequently confirmed by numerous experimenters. It states that the lowering of the freezing point, when one mole of various solutes is dissolved in the same arbitrarily selected quantity (100 grams) of a solvent, is a constant quantity. Hence it is evident that the right ...
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This historic book may have numerous typos and missing text. Purchasers can download a free scanned copy of the original book (without typos) from the publisher. Not indexed. Not illustrated. 1920 Excerpt: ...is the empirical formula obtained by him and g subsequently confirmed by numerous experimenters. It states that the lowering of the freezing point, when one mole of various solutes is dissolved in the same arbitrarily selected quantity (100 grams) of a solvent, is a constant quantity. Hence it is evident that the right-hand member of equation (1) must also represent this same constant. Therefore, knowing T, which is the temperature of the freezing point of the pure solvent, and LF, which is the latent 2 T2 heat of fusion of the pure solvent, the value of--can be 100 LF readily ascertained, which is the value of the gram-molecular lowering of the solvent. There is no term in this expression which relates to the dissolved substance, hence the character of the solute should not affect the value, and we are justified in drawing the conclusion that the gram-molecular lowering of the freezing point is a constant and independent of the solute, i.e. 2 = KF = = gram 100 LF g molecular lowering. We have then two experimental methods by means of which the value of this constant, KF, can be determined: (1) as Raoult did, by determining the lowering produced by the freezing point method, (2) as van't Hoff did, by calculating the value of KF from the latent heat of fusion of the solvent. The agreement between the two methods is very close, as the values in Table XLVII show, wherein the quantity of the solvent, S, employed is 100 grams. The value for the latent heat of fusion, LP, for nitrobenzene had not been determined, and van't Hoff calculated it from the value of KF, obtained experimentally and found it to be 22.1 calories per gram. Pettersson subsequently determined the latent heat and found it to be 22.3 calories. Similarly for ethyl bromide, from the value of KF t...
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Add this copy of Textbook of Physical Chemistry to cart. $69.86, good condition, Sold by Bonita rated 4.0 out of 5 stars, ships from Newport Coast, CA, UNITED STATES, published 2015 by Arkose Press.
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Add this copy of Textbook of Physical Chemistry to cart. $67.46, good condition, Sold by Bonita rated 4.0 out of 5 stars, ships from Newport Coast, CA, UNITED STATES, published 2010 by Nabu Press.