CBSE Class 12-science Answered
what is the relation between or how we can predict the spontaniety of hemical process based on the standard electrode potential value?
Asked by sofy shoukath | 08 Mar, 2013, 07:52: PM
Expert Answer
The spontaneity of a redox reaction is a function of the reduction potentials of the two species involved in the reaction: the reducing agent and the oxidizing agent.
To determine if a reaction is spontaneous or not, you must first isolate the two half-reactions. To do this, see the Related Questions link to the left "How do you balance a redox reaction?"
Once you have the two half-reactions, you must look at a table of standard potentials to find the values for the half-reactions occurring in the overall reaction in question. For a table of standard reduction potentials, see the Web Links to the left of this answer.
Standard potentials are almost always listed as reductions -- in other words the energy either require or released when an element gains an electron. However, a redox reaction always involves one species (an atom or molecule) gaining one or more electrons and another species losing one or more electrons. To convert a reduction potential into the opposite reaction, an oxidation reaction, just flip the direction of the arrow in the reaction and reverse the sign of the potential.
To determine if a reaction is spontaneous or not, you must first isolate the two half-reactions. To do this, see the Related Questions link to the left "How do you balance a redox reaction?"
Once you have the two half-reactions, you must look at a table of standard potentials to find the values for the half-reactions occurring in the overall reaction in question. For a table of standard reduction potentials, see the Web Links to the left of this answer.
Standard potentials are almost always listed as reductions -- in other words the energy either require or released when an element gains an electron. However, a redox reaction always involves one species (an atom or molecule) gaining one or more electrons and another species losing one or more electrons. To convert a reduction potential into the opposite reaction, an oxidation reaction, just flip the direction of the arrow in the reaction and reverse the sign of the potential.
Answered by | 09 Mar, 2013, 11:19: AM
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