Nickel-cadmium battery reaction

At another type of active electrode, found in many batteries, the reaction is the conversion between a metal and an Insoluble salt. At the surface of this type of electrode, metal cations combine with anions from the solution to form the salt. One example is the cadmium anode of a rechargeable nickel-cadmium battery, at whose surface cadmium metal loses electrons and forms cations. These cations combine immediately with hydroxide ions in... 

A redox half-reaction at an active electrode also may convert one metal salt into another. For example, the cathode In a nickel-cadmium battery is NiO(OH), which is reduced to nickel(II) hydroxide. The half-reaction reduces... 

The following half-reactions occur in the rechargeable nickel-cadmium battery ... 

The relatively simple chemistry of this redox reaction is one reason why nickel-cadmium batteries are rechargeable. As we show later in this chapter, applying an external voltage can reverse this reaction. 

C19-0095. After use, a nickel-cadmium battery has 1.55 g of Cd (OH)2 deposited on its anode. It is inserted in a recharger that supplies 125 inA of current at a voltage of 1.45 V. (a) To which electrode, Ni or Cd, should the negative wire from the charger be connected Write the half-reaction occurring at this electrode during charging, (b) Compute the time in hours needed to convert all 1.55 g of Cd (OH)2 back to Cd metal. 

Nickel(lll) oxide, prepared from a nickel(ii) salt and sodium hypochlorite, is used for the oxidation of alkanols in aqueous alkali [46]. Residual nickel(Ii) oxide can be re-activated by reaction with sodium hypochlorite. Nickel oxides have also long been used in the manufacture of the positive pole in the Edison nickel-iron rechargeable battery, now largely superseded by die lead-acid accumulator, and in the Jungner nickel-cadmium batteries used as button cells for calculators [47]. Here, prepared nickel oxide is pressed into a holding plate of perforated nickel. Such prepared plates of nickel(lli) oxide have been proposed as reagent for the oxidation, in alkaline solution, of secondary alcohols to ketones and primary alcohols to carboxylic acids [48]. Used plates can be regenerated by anodic oxidation. 

Write a balanced equation for the reaction that occurs when a nickel-cadmium battery is recharged. If 10.0 g of Ni(OH)2 is oxidized in the charging process, how many grams of cadmium are formed ... 

Lead-acid, nickel-iron (Ni-Fe), nickel-cadmium (NiCd), and nickel-metal hydride (NiMH) batteries are the most important examples of batteries with aqueous electrolytes. In lead-acid batteries, the overall electrochemical reaction upon discharge consists of a comproportionation of Pb° and Pb4+ to Pb2+. All nickel-containing battery reactions are based on the same cathodic reduction of Ni3+ to Ni2+, but utilize different anodic reactions providing the electrons. Owing to toxicity and environmental concerns, the formerly widely used Cd°/Cd2+ couple (NiCd cells) has been almost entirely replaced by H/H+, with the hydrogen being stored in a special intermetallic compound (NiMH). 

An especially important type of dry cell is the nickel-cadmium battery, in which the electrode reactions are as follows ... 

The nickel-cadmium battery is the most popular alkaline secondary battery. The cell and its reaction are ... 

Combining the nickel cadmium and nickel-hydrogen systems technologies has given rise to the nickel-metal hydride rechargeable battery, one of the most advanced rechargeable systems commercially available and an environmentally friendlier alternative to nickel-cadmium batteries. The cell and its reaction may be written ... 

Rechargeable batteries have become an essential part of our environmentally conscientious society. The nickel-cadmium cell battery is a rechargeable battery used in small electronic devices. The half reactions that take place in the nickel-cadmium battery during discharge are ... 

The reaction taking place at the anode when the nickel-cadmium batteries are discharging is ... 

When the nickel-cadmium battery is recharging, what is the reaction at the anode ... 

Nickel-cadmium batteries use a hydrate nickel oxide as positive electrode, a metallic cadmium as negative electrode and an aqueous solution of potassium hydroxide as electrolyte [17]. The production of electrons at the negative plate during discharge occurs via the following semi-reaction ... 

The nickel-cadmium battery (Ni-Cd) is the most common battery used in communication satellites, in Earth orbiters, and in space probes. The chemical reactions are ... 

SECTION 20.7 A battery is a self-contained electrochemical power source that contains one or more voltaic cells. Batteries are based on a variety of different redox reactions. Several common batteries were discussed. The lead-acid battery, the nickel-cadmium battery, the nickel-metal-hydride battery, and the lithium-ion battery are examples of rechargeable batteries. The common alkaline dry cell is not rechargeable. Fuel cells are voltaic cells that utilize redox reactions in which reactants such as H2 have to be continuously supplied to the cell to generate voltage. 

The cell voltage is 1.3 V. Eqs. (9.23) and (9.24) are formal equations the exact processes in the nickel-cadmium battery are complex solid-state reactions. More details and other types of batteries are described in special Uterature. ... 

In some apphcations nickel-cadmium batteries have been replaced by nickel-zinc batteries.The overall cell reaction for this relatively new battery is ... 

Figure 13.16 I Important design features of a nickel-cadmium battery-are shown. Transforming an electrochemical reaction into a useful consumer battery offers many engineering challenges.

Give the cathode, anode, and overall reactions when a nickel-cadmium battery is charged. 

See directions preceding Exercise 58.) A reaction is proposed for a nickel—cadmium battery as Ni(s) +... 

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