The mass of zinc produced by the electrolysis of zinc sulphate solution with a steady current of 0.015 A for 15 minutes is \_\_\_\_\_\_ times 10^-4$\_\_\_\_\_\_ \times 10^{-4}$ g. (Atomic mass of zinc = 65.4$= 65.4$ amu)

### Related Formula W = Z cdot I cdot t = fracMn cdot F cdot I cdot t$$W = Z \cdot I \cdot t = \frac{M}{n \cdot F} \cdot I \cdot t$$ where, W$W$ = mass deposited Z$Z$ = electrochemical equivalent I$I$ = current in amperes t$t$ = time in seconds M$M$ = molar mass n$n$ = n-factor (electrons exchanged) F$F$ = Faraday's constant (96500 text C/mol$96500 \text{ C/mol}$) ### Core Logic The electrolysis of zinc sulphate (ZnSO_4$ZnSO_4$) involves the reduction of zinc ions at the cathode: Zn^+2 + 2e^- rightarrow Zn$$Zn^{+2} + 2e^- \rightarrow Zn$$ Here, the n-factor (n$n$) is 2. ### Step 1: Calculation Given values: I = 0.015text A$I = 0.015\text{ A}$ t = 15text minutes = 15 times 60text seconds = 900text s$t = 15\text{ minutes} = 15 \times 60\text{ seconds} = 900\text{ s}$ M = 65.4text g/mol$M = 65.4\text{ g/mol}$ F approx 96500text C$F \approx 96500\text{ C}$ Plugging the values into Faraday's First Law: W = frac65.42 times 96500 times 0.015 times 15 times 60$$W = \frac{65.4}{2 \times 96500} \times 0.015 \times 15 \times 60$$ W = frac65.4193000 times 13.5$$W = \frac{65.4}{193000} \times 13.5$$ W = 3.3886 times 10^-4 times 13.5$$W = 3.3886 \times 10^{-4} \times 13.5$$ W = 45.746 times 10^-4text g$$W = 45.746 \times 10^{-4}\text{ g}$$ Rounding to two decimal places (or nearest integer depending on convention), we get 45.75 times 10^-4text g$45.75 \times 10^{-4}\text{ g}$. ### Evaluation Rubric / Model Answer null ### Chapter Mix Class 12 Chemistry: Electrochemistry