1e:I[80107,["/_next/static/chunks/235ad55241b6443f.js","/_next/static/chunks/8337ab1f037b6654.js","/_next/static/chunks/c9e933b5fd1a0afc.js","/_next/static/chunks/848a330faa2461ac.js","/_next/static/chunks/9f2942e368a262d2.js","/_next/static/chunks/92f9e11244990470.js","/_next/static/chunks/a8b867fbb1dfca1a.js","/_next/static/chunks/1100f0390a901fa7.js","/_next/static/chunks/bbe6bd9d3c7b0355.js","/_next/static/chunks/a82195c3e5de7dd4.js"],"default"] 1f:I[76763,["/_next/static/chunks/235ad55241b6443f.js","/_next/static/chunks/8337ab1f037b6654.js","/_next/static/chunks/c9e933b5fd1a0afc.js","/_next/static/chunks/848a330faa2461ac.js","/_next/static/chunks/9f2942e368a262d2.js","/_next/static/chunks/92f9e11244990470.js","/_next/static/chunks/a8b867fbb1dfca1a.js","/_next/static/chunks/1100f0390a901fa7.js","/_next/static/chunks/bbe6bd9d3c7b0355.js","/_next/static/chunks/a82195c3e5de7dd4.js"],"default"] 1d:T437,{"@context":"https://schema.org","@graph":[{"@type":"BreadcrumbList","itemListElement":[{"@type":"ListItem","position":1,"name":"Home","item":"https://www.divinejee.com"},{"@type":"ListItem","position":4,"name":"The logarithm of equilibrium constant for the reaction Pd24 ","item":"https://www.divinejee.com/question/the-logarithm-of-equilibrium-constant-for-the-reaction-pd2-4-cl-leftharpoons-pdcl42-is-nearest"}]},{"@type":"QAPage","mainEntity":{"@type":"Question","name":"Question The logarithm of equilibrium constant for the reaction Pd24 on Topic","text":"

The logarithm of equilibrium constant for the reaction $\\mathrm{Pd}^{2+}+4 \\mathrm{Cl}^{-} \\rightleftharpoons \\mathrm{PdCl}_{4}^{2-}$ is __________...","answerCount":1,"upvoteCount":0,"datePublished":"2026-01-16","author":{"@type":"Organization","name":"DivineJEE"},"acceptedAnswer":{"@type":"Answer","text":"Check the detailed solution on the page.","upvoteCount":0,"url":"https://www.divinejee.com/question/the-logarithm-of-equilibrium-constant-for-the-reaction-pd2-4-cl-leftharpoons-pdcl42-is-nearest"}}}]}20:T478,Sol. $\Delta G^{\circ}=-R T \ell n K$

$$ \begin{aligned} & -\mathrm{nFE}_{\text {cell }}^{\mathrm{o}}=-\mathrm{RT} \times 2.303\left(\log _{10} \mathrm{~K}\right) \\\\ & \frac{\mathrm{E}_{\text {Cell }}^{\mathrm{o}}}{0.06} \times \mathrm{n}=\log \mathrm{K} .......(1) \\\\ & \mathrm{Pd}^{+2} \text { (aq.) }+ \mathrm{2e}^{-} \rightleftharpoons \mathrm{Pd}(\mathrm{s}), \mathrm{E}_{\text {cat, }{ reduction}}^{\mathrm{o}}=0.83 \\\\ & \mathrm{Pd}(\mathrm{s})+4 \mathrm{Cl}^{-} \text {(aq.) } \rightleftharpoons \mathrm{PdCl}_4^{2-}, \text { (aq) }+2 \mathrm{e}^{-}, \mathrm{E}_{\text {Anode, Oxidation }}^0=0.65 \end{aligned} $$

Net Reaction $\rightarrow \mathrm{Pd}^{2+}$ (aq.) $+4 \mathrm{Cl}^{-}$(aq.) $\rightleftharpoons \mathrm{PdCl}_4^{2-}$ (aq.)

$$ \begin{aligned} & \mathrm{E}_{\text {cell }}^0=\mathrm{E}_{\text {cat,red }}^{\mathrm{o}}-\mathrm{E}_{\text {Anded, oxidid }}^0 \\\\ & \mathrm{E}_{\text {cell }}^{\mathrm{o}}=0.83-0.65 \\\\ & \mathrm{E}_{\text {cell }}^0=0.18 .........(2) \end{aligned} $$

Also $\mathrm{n}=2$ .......(3)

Using equation (1), (2) and (3)

$\log K=6$