Redox Reactions
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8 months agoContributor-Level 10
The potential associated with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any gas appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further there action is carried out at 298K, then the potential of each electrode is said to be the Standard Electrode Potential. By convention, the standard electrode potential (E? ) of hydrogen electrode is 0.00 volts. The electrode potential value for each electrode process is a measure of the relative tendency of the active species in the process to remainin the oxidised/reduced fo
New answer posted
8 months agoContributor-Level 10
Two methods are used to balance chemical equations for redox processes. One of these methods is based on the change in the oxidation number of reducing agent and the oxidising agent (i.e. oxidation number method) and the other method is based on splitting the redox reaction into two half reactions — one involving oxidation and the other involving reduction (half reaction method). Both these methods are in use and the choice of their use rests with the individual using them.
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8 months agoContributor-Level 10
(a) Combination reactions (b) Decomposition reactions (c) displacement reactions (d) Disproportionation reactions.
New answer posted
8 months agoContributor-Level 10
Electrochemical series is the series of elements in which elements are arranged in decreasing order of their reduction potential.
Reducing power goes on increasing whereas oxidising power goes on decreasing down the series.
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8 months agoContributor-Level 10
Electrochemical cell is a device in which the redox reaction is carried indirectly and the decrease in free energy appears as electrical energy.
At cathode there is gain of electrons.
At anode there is loss of electrons.
In electrochemical cell anode is written on L.H.S while cathode is written on R.H.S.
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8 months agoContributor-Level 10
(b) Oxidation involves gain of one or more electrons by a species during a reaction.
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8 months agoNew answer posted
8 months agoContributor-Level 10
(c) In ClO4–, chlorine is in maximum oxidation state of +7. So, it does not show the disproportionation reaction.
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8 months agoContributor-Level 10
(d) In H2O2 oxidation number of O = -1 and can vary from 0 to -2 (+2 is possible in OF2). The oxidation number can decrease or increase, because of this H2O2 can act both asoxidising and reducing agent.
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