A spontaneous redox reaction between two elements occurs when one element is oxidized (loses electrons) and another is reduced (gains electrons) without the need for external energy. This typically happens when the two elements have a significant difference in their standard reduction potentials, leading to a favorable energy change. The result is the formation of new products, often in the form of ions or compounds, along with the release of energy, such as heat or light. For example, the reaction between zinc and copper sulfate results in the spontaneous displacement of copper by zinc, producing zinc sulfate and copper metal.
The element with the greater reduction potential is the one that is reduced.
The reduction potential plus oxidation potential is negative.
The element with the greater reduction potential is the one that is reduced.
Which element will be oxidized and which will be reduced
In an electrolytic cell, an external power source is needed to drive a non-spontaneous redox reaction, while in a voltaic cell, the redox reaction is spontaneous and generates electric energy. In an electrolytic cell, the anode is positive and the cathode is negative, whereas in a voltaic cell, the anode is negative and the cathode is positive.
The element with the greater reduction potential is the one that is reduced.
The element with the greater reduction potential is the one that is reduced.
Which element will be oxidized and which will be reduced
spontaneous redox reaction
For a redox reaction to be spontaneous, the standard cell potential (cell) must be positive.
A redox reaction can be identified by the transfer of electrons between reactants. Look for changes in oxidation states of elements involved in the reaction to determine if it is a redox reaction.
. The reaction will be spontaneous.
A positive sum of the two half-reactions' standard potentials
oxidation
Which element will be oxidized and which will be reduced
The sum of the voltages of the half-reactions is positive.
The reduction potential plus oxidation potential is negative.