Physical Chemistry and Its Biological ApplicationsPhysical Chemistry and Its Biological Applications ... |
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Page 21
... observed P , ideal 1.000 10.04 1.000 10.00 50.0 200.0 50.8 193.1 1.000 0.999 10.00 50.0 200.0 9.97 49.3 182.5 Carbon dioxide Temperature 30 ° C 100 ° C P , observed 50.0 200.0 50.0 200.0 P , ideal 71.6 504.4 56.6 335.3 P , van der Waals ...
... observed P , ideal 1.000 10.04 1.000 10.00 50.0 200.0 50.8 193.1 1.000 0.999 10.00 50.0 200.0 9.97 49.3 182.5 Carbon dioxide Temperature 30 ° C 100 ° C P , observed 50.0 200.0 50.0 200.0 P , ideal 71.6 504.4 56.6 335.3 P , van der Waals ...
Page 372
... observed to increase with increasing buffer concentration , the reaction is said to be catalyzed by the acid CH , COOH or by the base CH , COO- or by both , as well as by H , O + . As might be expected , other acids show similar effects ...
... observed to increase with increasing buffer concentration , the reaction is said to be catalyzed by the acid CH , COOH or by the base CH , COO- or by both , as well as by H , O + . As might be expected , other acids show similar effects ...
Page 390
... observed a change in rate only of the order of 5 to 20 percent , and then only when the isotope is directly involved in the bond that undergoes a change in the reaction . Secondary isotope effects probably also exert their influence by ...
... observed a change in rate only of the order of 5 to 20 percent , and then only when the isotope is directly involved in the bond that undergoes a change in the reaction . Secondary isotope effects probably also exert their influence by ...
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absorption acid adsorbed adsorption amino amount behavior benzene Calculate carbon carboxyl cell chain charge Chem chemical chemical shift chloride cm³ coefficient complex components concentration containing corresponding curve described diagram dipole dissociation distance effect electric electrolyte electron energy change enthalpy entropy enzyme equal equation equilibrium constant example force free energy frequency function H₂O heat hydrogen atom hydrogen bonds increase interaction ionic ionization k₁ k₂ kcal kcal/mol kinetic magnetic field magnitude material measured membrane mixture molar mole fraction molecular weight molecules nuclei occurs orbital osmotic pressure oxidation oxygen particles polar potential protein proton quantum number radiation rate constant ratio reactant reaction represented resonance rotation sample shown in Figure sodium solid solubility solvent species spectrum spin structure substance sucrose surface tension temperature tion titration torr transition triplet tube vapor pressure velocity vibrational viscosity volume wavelength zero