Calculate emf of the half cell given below: Pt (s) | H₂$H_{2}$ (g, 2 atm) | HCl (aq, 0.02 M) E_H₂ / H⁺° = 0$$E_{H_{2} / H^{+}}^{\circ} = 0$$ (Given : 2.303 RTF = 0.059, 2 = 0.3010)$(\text{Given }: \frac{2.303 \mathrm{RT}}{\mathrm{F}} = 0.059, \log 2 = 0.3010)$

Related Formula

Core Logic

Cathode Reaction: Cu²⁺ + 2e⁻ arrow Cu(s)$Cu^{2+} + 2e^{-} \rightarrow Cu(s)$ Here, n = 2$n = 2$. Molar mass of Cu = 63 ~g mol⁻¹$63 \mathrm{~g \, mol}^{-1}$. Equivalent mass of Cu (E$E$) = (63)/(2) = 31.5 ~g eq⁻¹$= \frac{63}{2} = 31.5 \mathrm{~g \, eq}^{-1}$.

Given variables: Current (I$I$) = 1.5 A$1.5 \text{ A}$. Time (t$t$) = 10 minutes = 10 × 60 = 600 s$10 \text{ minutes} = 10 \times 60 = 600 \text{ s}$. Faraday (F$F$) approx = 96500 ~C$96500 \mathrm{~C}$.

Step 1: Calculate Mass

Pattern Recognition

Use W = (M · I · t)/(nF)$W = \frac{M \cdot I \cdot t}{nF}$. Never forget to convert time from minutes to seconds, and remember that Copper in Copper Sulphate (CuSO₄$CuSO_4$) is in the +2 state (n=2$n=2$).

Chapter Mix

Class 12 Chemistry: Electrochemistry