The temperature coefficient of the emf i.e., ( textdE/ textdt) = - 0.00065 text VK- 1 for the cell Cd|.CdCl2(1 M)|.|.AgCl(s)|.Ag at text25 texto textC . Calculate the entropy changes textÎS text298 textK for the cell reaction textCd + text2 textAgCl arrow textCd2 + + 2 textCl- + 2 textAg .

Question

The temperature coefficient of the emf i.e., ( textdE/ textdt) = - 0.00065 text VK- 1 for the cell Cd|.CdCl2(1 M)|.|.AgCl(s)|.Ag at text25 texto textC . Calculate the entropy changes textÎS text298 textK for the cell reaction textCd + text2 textAgCl arrow textCd2 + + 2 textCl- + 2 textAg . (A) -105.5 JK- 1 (B) -150.2 JK- 1 (C) -75.7 JK- 1 (D) -125.5 JK- 1

Tardigrade Admin · Accepted Answer

Δ S=+nF(d E/d t) =2× 96500× (- 0.00065) = - 125.5 textJK- 1

Q. The temperature coefficient of the emf i.e., $\frac{dE}{dt} = - 0.00065 VK^{- 1}$ for the cell $C d ∣ C d C l_{2} (1 M) ∣ ∣ A g Cl (s) ∣ A g$ at $25^{o} C$ . Calculate the entropy changes $ΔS 298 K$ for the cell reaction $Cd + 2 AgCl \to Cd^{2 +} + 2 Cl^{-} + 2 Ag$ .

$- 105.5 J K^{- 1}$

$- 150.2 J K^{- 1}$

$- 75.7 J K^{- 1}$

$- 125.5 J K^{- 1}$

$Δ S = + n F \frac{d E}{d t}$

$= 2 \times 96500 \times (- 0.00065)$

$= - 125.5 JK^{- 1}$

Q. The temperature coefficient of the emf i.e., dtdE​=−0.00065 VK−1 for the cell Cd∣CdCl2​(1M)∣∣AgCl(s)∣Ag at 25oC . Calculate the entropy changes ΔS298K for the cell reaction Cd+2AgCl→Cd2++2Cl−+2Ag .

−105.5JK−1

−150.2JK−1

−75.7JK−1

−125.5JK−1