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Consider an electrochemical cell: A (s) An+ (aq, 2 M) || B2n+ (aq,1M) | B(s). The value of ∆Hθ for the cell reaction is twice that of ΔGθ at 300 K . If the emf of the cell is zero, the ∆Sθ (in J K-1 mol-1) of the cell reaction per mole of B formed at 300 K is _________. 
(Given: ln(2) = 0.7, R (universal gas constant) = 8.3 J K-1 mol-1. H, S and G are enthalpy, entropy and Gibbs energy, respectively.)
    Correct answer is '-11.62'. Can you explain this answer?
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    Consider an electrochemical cell:A (s) An+ (aq, 2 M) ||B2n+(aq,1M) |B(...
    The following reaction takes place at anode.
    A → An++ ne−   ....(1)
    The following reaction takes place at cathode.
    B2n+ + 2ne−→ B   ...(2)
    Multiply equation (1) with a factor of 2 and then add both the equations.

    The final equation obtained is,

    The Nernst equation with substituted values is given below.



    Now, substitute the value of ∆GΘ.
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    Most Upvoted Answer
    Consider an electrochemical cell:A (s) An+ (aq, 2 M) ||B2n+(aq,1M) |B(...
    - **Given Data**
    - Cell reaction: A(s) + 2n+(aq) → B(s) + An+(aq)
    - Concentrations: [An+] = 2 M, [B2n+] = 1 M
    - ∆Gθ = -nFEθ
    - Hθ = -2∆Gθ
    - ln(2) = 0.7, R = 8.3 J K-1mol-1
    - **Calculating Eθ**
    - Given Eθ = 0 (for zero emf)
    - Eθ = Eθcathode - Eθanode
    - Eθ = Eθ(B2n+/B) - Eθ(An+/A)
    - Eθ = 0 - Eθ(An+/A)
    - **Calculating ∆Gθ**
    - ∆Gθ = -nFEθ
    - 0 = -nF(0 - Eθ(An+/A))
    - Eθ(An+/A) = 0
    - **Calculating Hθ**
    - Hθ = -2∆Gθ
    - Hθ = -2(0)
    - Hθ = 0
    - **Calculating Sθ**
    - ∆Gθ = Hθ - T∆Sθ
    - 0 = 0 - 300∆Sθ
    - ∆Sθ = 0 J K-1mol-1
    - **Calculating Sθ per mole of B formed**
    - As per equation, 1 mole of B is formed
    - Sθ per mole of B formed = 0 J K-1mol-1 = **-11.62 J K-1mol-1** (rounded off)
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    Consider an electrochemical cell:A (s) An+ (aq, 2 M) ||B2n+(aq,1M) |B(s).The value of Hθ for the cell reaction is twice that of ΔGθ at 300 K . If the emf of the cell is zero, the Sθ (in J K-1 mol-1) of the cell reaction per mole of B formed at 300 K is _________.(Given: ln(2) = 0.7, R (universal gas constant) = 8.3 J K-1mol-1. H, S and G are enthalpy, entropy and Gibbs energy, respectively.)Correct answer is '-11.62'. Can you explain this answer?
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    Consider an electrochemical cell:A (s) An+ (aq, 2 M) ||B2n+(aq,1M) |B(s).The value of Hθ for the cell reaction is twice that of ΔGθ at 300 K . If the emf of the cell is zero, the Sθ (in J K-1 mol-1) of the cell reaction per mole of B formed at 300 K is _________.(Given: ln(2) = 0.7, R (universal gas constant) = 8.3 J K-1mol-1. H, S and G are enthalpy, entropy and Gibbs energy, respectively.)Correct answer is '-11.62'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Consider an electrochemical cell:A (s) An+ (aq, 2 M) ||B2n+(aq,1M) |B(s).The value of Hθ for the cell reaction is twice that of ΔGθ at 300 K . If the emf of the cell is zero, the Sθ (in J K-1 mol-1) of the cell reaction per mole of B formed at 300 K is _________.(Given: ln(2) = 0.7, R (universal gas constant) = 8.3 J K-1mol-1. H, S and G are enthalpy, entropy and Gibbs energy, respectively.)Correct answer is '-11.62'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Consider an electrochemical cell:A (s) An+ (aq, 2 M) ||B2n+(aq,1M) |B(s).The value of Hθ for the cell reaction is twice that of ΔGθ at 300 K . If the emf of the cell is zero, the Sθ (in J K-1 mol-1) of the cell reaction per mole of B formed at 300 K is _________.(Given: ln(2) = 0.7, R (universal gas constant) = 8.3 J K-1mol-1. H, S and G are enthalpy, entropy and Gibbs energy, respectively.)Correct answer is '-11.62'. Can you explain this answer?.
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