Consider the figure and mark the correct option. A. Activation energy of forward reaction is `E_(1)+E_(2)` and product is less stable than reactant.B. Activation energy of forward reaction is `E_(1)+E_(2)` and product is more stable than reactant.C. Activation energy of both forward and backward reaction is `E_(1)+E_(2)` and reactant is more stable than product.D. Activation energy of backward reaction if `E_(1)` and product is more stable than reactant.

Consider the figure and mark the correct option. A. Activation energy

1.	Consider the figure and mark the correct option. A. Activation energy of forward reaction is `E_(1)+E_(2)` and product is less stable than reactant.B. Activation energy of forward reaction is `E_(1)+E_(2)` and product is more stable than reactant.C. Activation energy of both forward and backward reaction is `E_(1)+E_(2)` and reactant is more stable than product.D. Activation energy of backward reaction if `E_(1)` and product is more stable than reactant.
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If an element can exist in several oxidation states, it is convenient to display the reduction potentials corresponding to the various half reactions in diagrammatic from, known as Latimer diagram. The Latimer diagram for chlorine in acid solution is `Cl_(4)^(-)overset(+1.20V)toClO_(3)^(-)overset(+1.60V)toClO_(2)^(-)overset(+1.60V)to` `ClO^(-)overset(+1.67V)toCl_(2)overset(+1.36V)toCl^(-)` In basic solution is : `ClO_(4)^(-)overset(+0.37V)toClO_(3)^(-)overset(+0.30V)toClO_(2)^(-)overset(+0.68)to` `ClO^(-)overset(+0.42V)toCl_(2)overset(+1.36)toCl^(-)`. The standard potentials for two nonadjacent species can also be calculated by using the concept that `DeltaG^(@)` is an additive property but using potential is not an assitive property and `DeltaG^(@)=-nFx^(0),` If a given oxidation state is a the next higher oxidation state disproportionation can occur. The reverse of relative stabilities of the oxidation state can also be understood by drawing a graph of `DeltaG^(@)//F` against oxidation state, known as Frost diagram, Choosing the stability of zero oxidation state arbitrery as zero. The most stable oxidation state of a apecies lies lowest in the digram Disproportionation is spontaneous if the species lies above a straight line joining its two product species. Which of the following couple have same value of potential at pH = 0 and pH = 14?A. `(ClO_(4)^(-))/(ClO_(3)^(-))`B. `(ClO_(2)^(-))/(Cl_(2))`C. `(ClO^(-))/(Cl_(2))`D. `(Cl_(2))/(Cl^(-))`
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If an element can exist in several oxidation states, it is convenient to display the reduction potentials corresponding to the various half reactions in diagrammatic from, known as Latimer diagram. The Latimer diagram for chlorine in acid solution is `Cl_(4)^(-)overset(+1.20V)toClO_(3)^(-)overset(+1.60V)toClO_(2)^(-)overset(+1.60V)to` `ClO^(-)overset(+1.67V)toCl_(2)overset(+1.36V)toCl^(-)` In basic solution is : `ClO_(4)^(-)overset(+0.37V)toClO_(3)^(-)overset(+0.30V)toClO_(2)^(-)overset(+0.68)to` `ClO^(-)overset(+0.42V)toCl_(2)overset(+1.36)toCl^(-)`. The standard potentials for two nonadjacent species can also be calculated by using the concept that `DeltaG^(@)` is an additive property but using potential is not an assitive property and `DeltaG^(@)=-nFx^(0),` If a given oxidation state is a the next higher oxidation state disproportionation can occur. The reverse of relative stabilities of the oxidation state can also be understood by drawing a graph of `DeltaG^(@)//F` against oxidation state, known as Frost diagram, Choosing the stability of zero oxidation state arbitrery as zero. The most stable oxidation state of a apecies lies lowest in the digram Disproportionation is spontaneous if the species lies above a straight line joining its two product species. For a hypothetical element, the Frost diagram is shown in figure Which of the following oxidation state is least stable ?A. -1B. 0C. 2D. 3
If an element can exist in several oxidation states, it is convenient to display the reduction potentials corresponding to the various half reactions in diagrammatic from, known as Latimer diagram. The Latimer diagram for chlorine in acid solution is `Cl_(4)^(-)overset(+1.20V)toClO_(3)^(-)overset(+1.60V)toClO_(2)^(-)overset(+1.60V)to` `ClO^(-)overset(+1.67V)toCl_(2)overset(+1.36V)toCl^(-)` In basic solution is : `ClO_(4)^(-)overset(+0.37V)toClO_(3)^(-)overset(+0.30V)toClO_(2)^(-)overset(+0.68)to` `ClO^(-)overset(+0.42V)toCl_(2)overset(+1.36)toCl^(-)`. The standard potentials for two nonadjacent species can also be calculated by using the concept that `DeltaG^(@)` is an additive property but using potential is not an assitive property and `DeltaG^(@)=-nFx^(0),` If a given oxidation state is a the next higher oxidation state disproportionation can occur. The reverse of relative stabilities of the oxidation state can also be understood by drawing a graph of `DeltaG^(@)//F` against oxidation state, known as Frost diagram, Choosing the stability of zero oxidation state arbitrery as zero. The most stable oxidation state of a apecies lies lowest in the digram Disproportionation is spontaneous if the species lies above a straight line joining its two product species. Which of the following statement is correct according to above question ?A. `A^(+1)` undergoes disproportionation into A and `A^(2+)`B. `A^(2+)` undergoes disproportionation in A and `A^(3+)`C. A undergoes comproportionation into `A^(+1)` and `A^(-1)`D. All of the above
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