A hypothetical electrochemical cell is shown below
A- | A+ (xM)|| B+ (yM)|B+
The emf measured is +0.20 V. The cell reaction is:
A+ + B → A + B+
A+ + e- → A ; B+ + e- → B-
the cell reaction cannot be predicted
the cell reaction cannot be predicted
Concentration of the Ag+ ions in a saturated solution of Ag2C2O4 is 2.2 ×10–4 mol L–1. Solubility product
2.42 × 10–8
2.66 × 10–12
4.5 × 10–11
4.5 × 10–11
In the electrochemical cell :
Zn|ZnSO4(0.01M)||CuSO4(1.0 M)|Cu, the emf of this Daniel cell is E1. When the concentration of ZnSO4 is changed to 1.0 M and that of CuSO4 changed to 0.01 M, the emf changes to E2. From the following, which one is the relationship between E1 and E2?
(Given, RT/F= 0.059)
E1= E2
E1< E2
E1> E2
E1> E2
When a lead storage battery is discharged;
SO2 is evolved
lead sulphate is consumed
lead is formed
sulphuric acid is consumed
The value of reaction quotient [Q], for the following cell
Zn(s)|Zn2+ (0.01 M)|| Ag+ (1.25 M | Ag (s) is
156
125
1.25 x 10-2
6.4 x 10-3
The standard reduction potential for Zn2+/Zn, Ni2+/Ni and Fe2+/Fe are -0.76, -0.23 and -0.44 V, respectively.
The reaction X + Y2+ → X2+ + Y will be spontaneous when
X = Ni, Y = Fe
X = Ni, Y = Zn
X =Fe, Y = Zn
X = Zn, Y = Ni
For the cell reaction,
Pb + Sn2+ Pb2+ + Sn
Given that, Pb Pb2+, E = 0.13 V
Sn2+ +2e- Sn, E = -0.14 V
What would be the ratio of cation concentration for which E = 0 ?
In the reaction,
X + I2 + 2HCl SnCl4 + 2HI
The correct option regarding X is/ are
It is an strong reducing agent
It is an angular molecule
It is used as a reagent in test of Hg2+ radical
All of the above
D.
All of the above
In the above given equation, X is represented by SnCl2. The complete equation can be written as-
SnCl2 + I2 + 2HCl SnCl4 + 2HI
SnCl2 is a strong reducing agent because it is readily oxidised into Sn4+ ion. Since, Sn-atom in SnCl2 is sp2 -hybridised. So, it is an angular molecule. On the other hand, it is used as a reagent in test of Hg2+ radical.
The E values for Mn and Zn are more negative than expected because
they have either half-filled and fully-filled configurations
they can easily donate electrons
it is quite easy to remove electrons from their orbitals
None of the above
When an iron object is plated with tin, tin does not act as sacrificial anode in protecting against corrosion, because
tin is more reactive than iron
tin is less reactive than iron
reactivity of tin and iron is same
tin is oxidising agent while iron is not so