Silver . calculations

B. Adsorption isotherm of Pseudocyanine in colloidal silver calculated from the spectral data of Figure 4A. See text for details... 

Fig. 11 Theoretical simulation of sensing action using EOT through nanoslits in silver calculated using the rigorous coupled-wave approach...

The limiting reactant must be identified because it will determine the amount of silver produced. To find the limiting reactant, we calculate the theoretical amount of silver produced by each reactant. The reactant that will produce the smallest mass of silver is the limiting reactant, and the mass of silver calculated for it is the amount produced by the reaction. 

From this example and the silver calculations, it should be clear how the rest of the lines in Figure 12-5 were found. We have made several approximations. Where lines b and g meet, the (Fe " ) and the (Fe " ) are both below their maximum values, so that a slight curvature of these lines should exist close to this intersection. Such species as FeOH, Fe(OH)2, Fe203, and Fe304 have been ignored. Nevertheless, the diagram will allow interpretations of iron chemistry such as the following ... 

Tarazona A, Kreisig S, Koglin E and Schwuger M J 1997 Adsorption properties of two cationic surfactant classes on silver surfaces studied by means of SERS spectroscopy and ab initio calculations Prog. Colloid Polym. Sol. 103 181-92... 

Let us suppose it is desired to calculate the theoretical yield of ethyl maleate when 33 g. of silver maleate, suspended m dry ether, are treated with the calculated quantity of ethyl iodide (31-2 g.). 

The method is generally applicable when other modes of esterification are either slow, inefficient, or likely to cause isomerisation it is, however, time-consuming and expensive. Small quantities of acid impurities are sometimes produced, hence it is advisable to wash the ester with saturated sodium bicarbonate solution. The silver salt can usually be prepared by dissolving the acid in the calculated quantity of standard ammonium hydroxide solution and... 

Preparation of silver maleate. Dissolve 65 g. of pure maleic acid (Section 111,143) in the calculated quantity of carefully standardised 3-5N aqueous ammonia solution in a 1-htre beaker and add, whilst stirring mechanically, a solution of 204 g. of silver nitrate in 200 ml. of water. Filter oflf the precipitated silver maleate at the pump, wash it with distilled water, and press well with the back of a large flat glass stopper. Dry in an electric oven at 50-60° to constant weight. The yield of the dry silver salt is 150 g. Store in a vacuum desiccator in the dark. 

Gravimetric factors are based on the 1993 International Atomic Weights. The factor Ag 0.7526 given in the first line of the table indicates that the weight of precipitate obtained (AgCl) is to be multiplied by 0.7526 to calculate the corresponding weight of silver. 

The sodium carbonate content may be deterrnined on the same sample after a slight excess of silver nitrate has been added. An excess of barium chloride solution is added and, after the barium carbonate has setded, it is filtered, washed, and decomposed by boiling with an excess of standard hydrochloric acid. The excess of acid is then titrated with standard sodium hydroxide solution, using methyl red as indicator, and the sodium carbonate content is calculated. 

A silver replica of a holly leaf is to be made by investment casting. (A natural leaf is coated with ceramic slurry which is then dried and fired. During firing the leaf burns away, leaving a mould cavity.) The thickness of the leaf is 0.4 mm. Calculate the liquid head needed to force the molten silver into the mould cavity. It can be assumed that molten silver does not wet the mould walls. 

Much later (Marcinkowsky and Berty 1973) it was proven that ethane did indeed have an effect. In the study of the inhibitor action of chlorinated hydrocarbons it was discovered that these compounds chlorinate the silver catalyst and ethane removes the chlorine from the catalyst by forming ethyl chloride. Since the inhibitor was in the 10 ppm range and similar quantities were used from the ethane present in about one volume percent, the small difference could not be calculated from material balance. The effect of ethane was only noticed as significant by the statistics, which justifies the statement made by Aris (1966) that, The need for sophistications should not be rejected unsophisticatedly. ... 

Using the data obtained from the silver nitrate experiments, we have derived a simple approximation to calculate the cavity polarisability as a function of diameter [22]. If we apply this model to cobalt nitrate, the derived threshold for filling is 0.8 nm [32] this result qualitatively agrees with our observations that cobalt nitrate-filled cavities are much narrower ( 2 nm) than obtained with silver nitrate (= 4 nm). 

II. The change of the sign between these two models may be also important for clustering and the surface growth mechanism. In the selfconsistent theory, the silver atoms tend to establish bonds with palladium atoms, while in the non-selfconsistent theory, the Ag-Ag bonds are favored. This explains the differences between the concentration profiles calculated within the models I and II and the fact that they do not simply follow the variations of the on-site terms. 

The button cells that provide the energy for watches, electronic calculators, hearing aids, and pacemakers are commonly alkaline systems of the silver oxide-zinc or mercuric oxide-zinc variety. These alkaline systems provide a vei y high energy density, approximately four times greater than that of the alkaline zinc-manganese dioxide battery. 

Chlorinity When a sample of sea water is titrated with silver nitrate, bromides and iodides, as well as chlorides are precipitated. In calculating the chlorinity (Cl), the entire halogen content is taken as chloride, and chlorinity is defined as the weight in grams of silver required for precipitation of total halogen content per kilogram of sea water, multiplied by 0-328 533. (Chlorinity is always expressed as parts per thousand, using the symbol %o.)... 

By x-ray diffraction it is possible to determine the geometric pattern in which atoms are arranged in a crystal and the distances between atoms. In a crystal of silver, four atoms effectively occupy the volume of a cube 0.409 nm on an edge. Taking the density of silver to be 10.5 g/cm3, calculate the number of atoms in one mole of silver ... 

Reality Check In FCC unit cells, the fraction of empty space is 0.26. When this is factored into the above, the calculated density of silver becomes 14.3 — (0.26)(14.3) =... 

Calculate the solubility (in grams per liter) of silver chloride in the following. 

This is because the concentrations of solid copper and solid silver are incorporated into the equilibrium constant. The concentration of solid copper is fixed by the density of the metal—it cannot be altered either by the chemist or by the progress of the reaction. The same is true of the concentration of solid silver. Since neither of these concentrations varies, no matter how much solid is added, there is no need to write them each time an equilibrium calculation is made. Equation (21) will suffice. 

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