For the reaction `2CI F_(3)(g) harr CI_(2)(g) +3F_(2)(g) log K_(eq) vs (1)/(T)` (where temperature is in K) curve is obtained as given. Which of the following change will increase the concentration of `CI_(2)` in an equilibrium mixture of `CI_(2), F_(2)` and `CIF_(3)`? A. Addition of inert gas at constant pressureB. Increase in temperature at constant volumeC. Addition of catalyst at equilibriumD. Removal of `F_(2)(g)` at equilibrium

For the reaction `2CI F_(3)(g) harr CI_(2)(g) +3F_(2)(g) log K_(eq) vs

1.	For the reaction `2CI F_(3)(g) harr CI_(2)(g) +3F_(2)(g) log K_(eq) vs (1)/(T)` (where temperature is in K) curve is obtained as given. Which of the following change will increase the concentration of `CI_(2)` in an equilibrium mixture of `CI_(2), F_(2)` and `CIF_(3)`? A. Addition of inert gas at constant pressureB. Increase in temperature at constant volumeC. Addition of catalyst at equilibriumD. Removal of `F_(2)(g)` at equilibrium
Answer» Correct Answer - B::D

Discussion

No Comment Found

Related InterviewSolutions

According to collision theory for determining the variation of rate of reaction with temperature the rate constant,`k= Ae^(-Ea//RT).` For most of the practical purposes A and `E_(a`[Arrhenius factor and Activation energy] are temperature independent. However they may vary slightly. Assuming the conditions given above answer the following questions. For constant A and `E_(a),` which parameters when plotted will give a straight line with given slope?A. `"ln k vs T ,Slope" = (E_(a))/(R)`B. `"ln k vs" 1/T "slope" = (E_(a))/(R)`C. `"ln k vs"1/T,"slope"=(E_(a))/(R)`D. `"ln k vs" T,"slope"=(E_(a))/(R)`
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^(-))`
According to the phase diagram shown, where does a mixture of solid and liquid exist at equilibrium ? A. Along line MNB. Along line KNC. Along line LND. In the region KNL
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
According to this phase diagram, which phases can exist at pressure lower than the triple point pressure ? A. Gas onlyB. Solid and gas onlyC. Liquid onlyD. Solid and liquid only
Observe the P-T phase diagram for a given substance A. Then melting point of `A(s)`, boiling point of `A(l)`, critical point of A and triple point of A (at their respective pressure) are respectively: A. `T_(1),T_(2),T_(3),T_(4)`B. `T_(4),T_(3),T_(1),T_(2)`C. `T_(3),T_(4),T_(2),T_(1)`D. `T_(2),T_(1),T_(3),T_(4)`
What is the normal boiling point of the solution represented by the phase diagram ? A. AB. BC. CD. D
What is the normal freezing point of the solution represented by the phase diagram ? A. `T_(1)`B. `T_(2)`C. `T_(3)`D. `T_(0)`
The curve represents the titration of : A. a diprotic acidB. two monoprotic acids with the same `K_(a^(s))` but different concentrations.C. two monoprotic acid with different `K_(a^(s))` but the same concentrationsD. two monoprotic acids with different `K_(a^(s))` and different concentrations.

Discussion

No Comment Found

Related InterviewSolutions

Reply to Comment