Silver metal reactions with

Another common reference cell found in the chemical-processing industry and useful in organic electrochemistry is the silver/silver chloride half-cell. The cell consists of silver metal coated with a paste of silver chloride immersed in an aqueous solution sam-rated with KCl and AgCl. The half-cell reaction is... 

PD is an aqueous solution containing silver ions, a ferrous/ferric redox (reduction/oxidation) system, a buffer (citric acid), and a cationic surfactant (generally -dodecylamine acetate). The ferrous (Fe ) ions in solution reduce the silver (Ag +) ions to silver metal (Ag°), with ferric (Fe + ) ions being present to hold back the reaction (eqn [1]) ... 

Silver metal reacts with nitric acid to give silver ion and nitric oxide. Write the balanced equation for this reaction. 

The chemical process examined has involved reaction with silver salts, and involves the transient formation of a silver-polymer adduct which immediately decomposes to yield the polymer radical and silver metal (reactions 4 and 5), the radical then copolymerizing the second monomer also present in the system. ... 

The darkening reaction involves the formation of silver metal within the silver haUde particles containing traces of cuprous haUde. With the formation of metallic silver, cuprous ions are oxidized to cupric ions (1,4). The thermal or photochemical (optical bleaching) reversion to the colorless or bleached state corresponds to the reoxidation of silver to silver ion and the reduction of cupric ion to reform cuprous ion. 

Fig. 9. Corrosion model of silver development. As the haUde ion, X, is removed into solution at the etch pit, the silver ion,, travels interstitiaHy, Ag/ to the site of the latent image where it is converted to silver metal by reaction with the color developer, Dev. Dev represents oxidized developer.

More general procedures for additions of halogen fluorides to highly fluori-nated olefins involve reactions with a source of nucleophilic fluoride ion, such as an alkali metal fluoride, in the presence of aposttive halogen donor [62 107, lOff, 109, 110, 111] (equations 11 and 12) These processes are likely to occur by the generation and capture of perfluorocarbamonic intermediates Tertiary fluormated carbanions can be isolated as cesium [112], silver [113], or tns(dimethylamino)sul-... 

In the reactions of 10.13a with alkali metal terr-butoxides cage expansion occurs to give the sixteen-atom cluster 10.15, in which two molecules of MO Bu (M = Na, K) are inserted into the dimeric structure. The cluster 10.13a also undergoes transmetallation reactions with coinage metals. For example, the reactions with silver(I) or copper(I) halides produces complexes in which three of the ions are replaced by Ag" or Cu" ions and a molecule of lithium halide is incorporated in the cluster. ... 

Not all metals react with aqueous acids. Among the common metals, magnesium, aluminum, iron, and nickel liberate H2 as zinc does. Other metals, including copper, mercury, silver, and gold, do not produce measurable amounts of hydrogen even though we make sure that the equilibrium state has been attained. With these metals, hydrogen is not produced and it is surely not just because of slow reactions. Apparently... 

These reactions can be viewed as a competition between two kinds of atoms (or molecules) for electrons. Equilibrium is attained when this competition reaches a balance between opposing reactions. In the case of reaction (3), copper metal reacting with silver nitrate solution, the Cu(s) releases electrons and Ag+ accepts them so readily that equilibrium greatly favors the products, Cu+2 and Ag(s). Since randomness tends to favor neither reactants nor products, the equilibrium must favor products because the energy is lowered as the electrons are transferred. If we regard reaction (5) as a competition between silver and copper for electrons, stability favors silver over copper. 

The negative voltage shows that the state of equilibrium favors the reactants more than the products for the reaction as written. For standard conditions, the reaction will not tend to occur spontaneously. However, if we place Ag(s) in 1 M H+, the Ag+ concentration is not 1 M— it is zero. By Le Chatelier s Principle, this increases the tendency to form products, in opposition to our prediction of no reaction. Some silver will dissolve, though only a minute amount because silver metal releases electrons so reluctantly compared with H2. It is such a small amount, in fact, that no silver chloride precipitate forms, even though silver chloride has a very low solubility. 

How many grams of silver metal will react with 2.0 liters of 6.0 M HNO3 The reaction is... 

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