ΔrG⊖=−nFEcell ⊖ For the given reaction, n=2 ∴ΔrG⊖=−2×96487×0.32 =−61751.68 J mol−1 =−61.751 kJ mol−1
NEET UG 2024 — Chemistry Physical Chemistry
The standard cell potential of the following cell ZnZn2+(aq)Fe2+(aq)∣Fe is 0.32 V . Calculate the standard Gibbs energy change for the reaction : Zn(s)+Fe2+(aq)→Zn2+(aq)+Fe(s) (Given : 1 F=96487C )
Held on 30 Apr 2024 · Verified 9 Jul 2026.
−61.75 kJ mol−1
+5.006 kJ mol−1
−5.006 kJ mol−1
+61.75 kJ mol−1
Sign in to track your attempts and accuracy.
Sign in to keep a private note on this question. Nothing you write is ever public.
The unit of rate constant for a first-order reaction is:
For the reaction 2SO₂(g) + O₂(g) ⇌ 2SO₃(g), ΔH = -198 kJ. Which condition favours forward reaction?
The standard heat of formation, in $\mathrm{kcal} / \mathrm{mol}^{\text {of }} \mathrm{Ba}^{2+}$ is : [Given : standard heat of formation of $\mathrm{SO}_4^{2-}$ ion (aq) $=-216 \mathrm{kcal} / \mathrm{mol}$, Standard heat of crystallisation of $\mathrm{BaSO}_4(\mathrm{~s})=-4.5 \mathrm{kcal} / \mathrm{mol}$, standard heat of formation of $\left.\mathrm{BaSO}_4(\mathrm{~s})=-349 \mathrm{kcal} / \mathrm{mol}\right]$
Match List - I with List - II $\begin{array}{llll} & \begin{array}{l} \text { List-I } \\ \text { (Example) } \end{array} & & \begin{array}{l} \text { List-II } \\ \text { (Type of Solution) } \end{array} \\ \text { A. } & \text { Humidity } & \text { I. } & \text { Solid in solid } \\ \text { B. } & \text { Alloys } & \text { II. } & \text { Liquid in gas } \\ \text { C. } & \text { Amalgams } & \text { III. } & \text { Solid in gas } \\ \text { D. } & \text { Smoke } & \text { IV. } & \text { Liquid in solid } \end{array}$ Choose the correct answer from the options given below:
The conjugate base of H₂SO₄ is:
Work through every NEET UG Physical Chemistry PYQ, year by year.