ElectrochemistryHard
Question
The EMF of the cell: Zn−Hg (C1M)|Zn2+ (aq)|Zn−Hg (C2M) at 25°C, if the concentrations of the zinc amalgams are: C1 = 10 g per 100 g of mercury, C2 = 1 g per 100 g mercury, is
Options
A.0.059 V
B.0.0295 V
C.0.59 V
D.0.295 V
Solution
Net cell reaction: Zn – Hg(C1M) ? Zn – Hg(C2M)
$E_{cell} = 0 - \frac{0.059}{2}.\log\frac{C_{2}}{C_{1}} = - \frac{0.059}{2}\log\frac{1}{10} = 0.0295\text{ V}$
Create a free account to view solution
View Solution FreeMore Electrochemistry Questions
Four colourless salt solutions are placed in separate test tubes and a strip of copper is placed in each. Which solution...If the pressure of hydrogen gas is increased from 1 atm. to 100 atm, keeping the hydrogen ion concentration constant at ...If a spoon of copper metal is placed in a solution of ferrous sulphate -...The passage of electricity in the Daniel cell when Zn and Cu electrodes are connected...Assertion :- BeSO4 is more soluble in water than BaSO4.Reason :- In BeSO4 H.E. exceeds its L.E....