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When Cl2 is dissolved in water , it disproportionate producing chloride ion and HClO. find in what hydronium ion concentration the potential for the disproportionation changes from negative value to a positive value , assuming 1.0 atm pressure and concentration of 1.0M for all species except hydronium ions . Given E(standard) (Cl2|Cl- ) =1.36V E(standard) (HClO2|Cl2) = 1.63V at 25 degree C?
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When Cl2 is dissolved in water , it disproportionate producing chlorid...
Introduction
When Cl2 is dissolved in water, it undergoes disproportionation producing chloride ions and HClO. The potential for the disproportionation changes from a negative value to a positive value at a certain hydronium ion concentration. This concentration can be calculated using the given standard electrode potentials.
Calculating the Equilibrium Constant
The disproportionation reaction of Cl2 is given by:
Cl2 + H2O ⇌ HClO + Cl-
The standard electrode potentials of the half-reactions involved are given as:
E(standard) (Cl2|Cl- ) = 1.36V
E(standard) (HClO2|Cl2) = 1.63V
Using these values, we can calculate the standard potential for the overall reaction:
E(standard) (HClO|Cl- ) = E(standard) (HClO2|Cl2) - E(standard) (Cl2|Cl- )
E(standard) (HClO|Cl- ) = 1.63V - 1.36V
E(standard) (HClO|Cl- ) = 0.27V
The standard potential for the overall reaction can be related to the equilibrium constant (K) using the Nernst equation:
E = E(standard) - (RT/nF)lnK
At 25°C, R = 8.314 J/mol·K, T = 298 K, n = 2 (number of electrons transferred), and F = 96,485 C/mol. Therefore, the equation becomes:
E = 0.27V - (RT/2F)lnK
Calculating the Hydronium Ion Concentration
The potential for the disproportionation changes from a negative value to a positive value when the equilibrium constant (K) is equal to 1. This occurs when the concentration of H3O+ ions reaches a certain value. To calculate this value, we can rearrange the equation above to solve for the hydronium ion concentration ([H3O+]):
lnK = (2F/RT)(E(standard) - E) + ln[H3O+]
ln(1) = (2F/RT)(0.27V - E) + ln[H3O+]
0 = (2F/RT)(0.27V - E) + ln[H3O+]
[H3O+] = e^(-(2F/RT)(0.27V - E))
Substituting the given values, we get:
[H3O+] = e^(-(2 × 96,485 C/mol)/(8.314 J/mol·K × 298 K) × (0.27V - E))
When the potential for the disproportionation changes from a negative value to a positive value, E = 0. Therefore, the hydronium ion concentration at this point is:
[H3O+] = e^(-(2 × 96,485 C/mol)/(8.314 J/mol·K × 298 K) × (0.27V - 0))
[H3O+] = 1.16 × 10^-4 M
Conclusion
The hydronium ion concentration at which the potential for the disproportionation of Cl
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When Cl2 is dissolved in water , it disproportionate producing chloride ion and HClO. find in what hydronium ion concentration the potential for the disproportionation changes from negative value to a positive value , assuming 1.0 atm pressure and concentration of 1.0M for all species except hydronium ions . Given E(standard) (Cl2|Cl- ) =1.36V E(standard) (HClO2|Cl2) = 1.63V at 25 degree C?
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When Cl2 is dissolved in water , it disproportionate producing chloride ion and HClO. find in what hydronium ion concentration the potential for the disproportionation changes from negative value to a positive value , assuming 1.0 atm pressure and concentration of 1.0M for all species except hydronium ions . Given E(standard) (Cl2|Cl- ) =1.36V E(standard) (HClO2|Cl2) = 1.63V at 25 degree C? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about When Cl2 is dissolved in water , it disproportionate producing chloride ion and HClO. find in what hydronium ion concentration the potential for the disproportionation changes from negative value to a positive value , assuming 1.0 atm pressure and concentration of 1.0M for all species except hydronium ions . Given E(standard) (Cl2|Cl- ) =1.36V E(standard) (HClO2|Cl2) = 1.63V at 25 degree C? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for When Cl2 is dissolved in water , it disproportionate producing chloride ion and HClO. find in what hydronium ion concentration the potential for the disproportionation changes from negative value to a positive value , assuming 1.0 atm pressure and concentration of 1.0M for all species except hydronium ions . Given E(standard) (Cl2|Cl- ) =1.36V E(standard) (HClO2|Cl2) = 1.63V at 25 degree C?.
When Cl2 is dissolved in water , it disproportionate producing chloride ion and HClO. find in what hydronium ion concentration the potential for the disproportionation changes from negative value to a positive value , assuming 1.0 atm pressure and concentration of 1.0M for all species except hydronium ions . Given E(standard) (Cl2|Cl- ) =1.36V E(standard) (HClO2|Cl2) = 1.63V at 25 degree C? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about When Cl2 is dissolved in water , it disproportionate producing chloride ion and HClO. find in what hydronium ion concentration the potential for the disproportionation changes from negative value to a positive value , assuming 1.0 atm pressure and concentration of 1.0M for all species except hydronium ions . Given E(standard) (Cl2|Cl- ) =1.36V E(standard) (HClO2|Cl2) = 1.63V at 25 degree C? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for When Cl2 is dissolved in water , it disproportionate producing chloride ion and HClO. find in what hydronium ion concentration the potential for the disproportionation changes from negative value to a positive value , assuming 1.0 atm pressure and concentration of 1.0M for all species except hydronium ions . Given E(standard) (Cl2|Cl- ) =1.36V E(standard) (HClO2|Cl2) = 1.63V at 25 degree C?.
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