Given the data at 25°C,
Ag + I– → AgI + e– ; E° = 0.152 V
Ag → Ag+ + e–; E° = –0.800 V
What is the value of log Ksp for AgI? $\left(2.303dfrac{ ext{RT}}{ ext{F}} = 0.059 ext{ V} ight)$
Given the data at 25°C,
Ag + I– → AgI + e– ; E° = 0.152 V
Ag → Ag+ + e–; E° = –0.800 V
What is the value of log Ksp for AgI? $\left(2.303dfrac{ ext{RT}}{ ext{F}} = 0.059 ext{ V} ight)$
The quantity of electricity needed to separately electrolyze 1 M solution of ZnSO4, AlCl3 and AgNO3 completely is in the ratio of |
Answer |
An infinite dilution of aqueous solution of BaCl2, molar conductivity of Ba2+ and Cl– ions are = 127.32 S cm2/moland 76.34 S cm2/mol respectively. What is Λ∞ |
Answer |
Aqueous copper sulphate solution is electrolyzed using platinum electrodes. The electrode reaction occurring at cathode is |
Answer |
Zn | Zn2+ (a = 0.1M) || Fe2+ (a = 0.01M) | Fe. The emf of the above cell is 0.2905 V. Equilibrium constant for the cell reaction is |
Answer |
Calculate the reduction potential of a half–cell containing platinum electrode immersed in 2.0 M Fe2+ and 0.02 M Fe3+. Given Eo Fe3+ + e– → Fe2+ |
Answer |
Consider the following four electrodes, P = Cu2+ (0.0001 M) | Cu(s) Q = Cu2+ (0.1 M) | Cu(s) R = Cu2+ (0.01 M) | Cu(s) S = Cu2+ (0.001 M) | Cu(s) If the standard reduction potential of Cu2+/Cu is +0.34 V, the reduction potentials in volts of the above electrodes follow the order |
Answer |
Conductivity of 0.01 M NaCl solution is 0.00147 ohm–1cm–1. What happens to this conductivity if extra 100 ml of H2O will be added to the above solution? |
Answer |
Cr2O2– EѲ |
Answer |
How many moles of Pt may be deposited on the cathode when 0.80 F of electricity is passed through a 1.0 M solution of Pt4+? |
Answer |
One ampere of current is passed for 9650 seconds through molten AlCl3. What is the weight in grams of Al deposited at cathode? (Atomic weight of Al = 27) |
Answer |