ElectrochemistryHard
Question
A galvanic cell is set up from a zinc bar weighing 100 g and 1.0 L of 1.0 M copper sulphate solution. How long would the cell run if it is assumed to deliver a steady current of 1.0 A? (Zn = 65.4)
Options
A.53.6 h
B.26.8 h
C.81.97 h
D.40.99 h
Solution
neq of Zn = $\frac{100}{65.4} \times 2 = 3.058$
neq of CuSO4 = $1.0 \times 2 = 2.0\left( \text{L.R.} \right)$
$\because n_{eq} = \frac{Q}{F} \Rightarrow 2 = \frac{1.0 \times t}{96500} $$$\Rightarrow t = 193000\text{ sec = 53.6 hr}$$
Create a free account to view solution
View Solution FreeMore Electrochemistry Questions
Given standard electrode potentials : Fe3+ + 3e- → Fe ; Eo = - 0.036 voltFe2+ + 2e- → Fe; Eo = - 0.440 volt ...Which cannot displace hydrogen from its compound ?...Calculate $\Lambda_{m}^{\infty}$ (in Ω−1 cm2 mol−1) for SrCl2 at 25°C, from the following data:Conc. 0.25 M 1.0 MΛm (in ...ASelect the correct statement about product A....For the reduction of NO3− ion in an aqueous solution, E° is +0.96 V. Values of E° for some metal ions are given below: V...