Advertisements
Advertisements
प्रश्न
E°cell for the given redox reaction is 2.71 V
Mg(s) + Cu2+ (0.01 M) → Mg2+ (0.001 M) + Cu(s)
Calculate Ecell for the reaction. Write the direction of flow of current when an external opposite potential applied is
(i) less than 2.71 V and
(ii) greater than 2.71 V
Advertisements
उत्तर
Ecell = `"E"°_"cell" - (0.0591)/(n)log ["Mg"^(2+)] // ["Cu"^(2+)]`
= `2.71 - (0.0591)/(2)log (0.001)/(0.01)`
=`2.71 - 0.0295 xx (-1)`
= `2.7395 "V"`
i) When an external potential is less than 2.71 then current will flow from copper to magnesium.
ii) When an external potential is greater than 2.71 then current will flow from magnesium to copper.
APPEARS IN
संबंधित प्रश्न
Can you store copper sulphate solutions in a zinc pot?
Among Zn and Cu, which would occur more readily in nature as metal and which as an ion?
Define the following term:
Fuel cell
A solution of Cu(NO3)2 is electrolyzed between platinum electrodes using 0.1 Faraday electricity. How many moles of Cu will be deposited at the cathode?
Define cathode
Can Fe3+ oxidises bromide to bromine under standard conditions?
Given: \[\ce{E^0_{{Fe^{3+}|Fe^{2+}}}}\] = 0.771 V
\[\ce{E^0_{{Br_{2}|Br^-}}}\] = −1.09 V
Is it possible to store copper sulphate in an iron vessel for a long time?
Given: \[\ce{E^0_{{Cu^{2+}|{Cu}}}}\] = 0.34 V and \[\ce{E^0_{{Fe^{2+}|{Fe}}}}\] = −0.44 V
The quantity of charge required to obtain one mole of aluminium from Al2O3 is ______.
The electrochemical cell stops working after some time because
The number of moles of electrons passed when the current of 2 A is passed through a solution of electrolyte for 20 minutes is ______.
