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Which of the following solutions has the highest
equivalent conductance?
1. 0.01 M NaCl
2. 0.05 M NaCl
3. 0.005 M NaCl
4. 0.02 M NaCl

A solution of Na₂SO₄ in water is electrolysed
using pt electrodes. The products at the cathode
and anod are respectively
1. H₂, SO₂
2. O₂, NaOH
3. H₂, O₂
4. O₂, SO₂

The reduction potential of the two half cell
reactions (occuring in an electrochemical cell)
are
PbSO₄(s) + 2e^– $\to$ Pb(s) + ${\mathrm{SO}}_4^{2-}$(aq) (E°= –0.31V)
Ag⁺(aq) + e^– $\to$ Ag(s) (E° = 0.80V)
The feasible reaction will be
1. Pb(s) + ${\mathrm{SO}}_4^{2-}$(aq) + 2 Ag⁺(aq)$\to$  2Ag (s) + PbSO₄ (s)
2. PbSO₄(s) + Ag⁺ (aq) $\to$ Pb(s)+${\mathrm{SO}}_4^{2-}$(aq) + 2Ag(s)
3. Pb(s) + ${\mathrm{SO}}_4^{2-}$ (s) + Ag(s) $\to$Ag⁺(aq) + PbSO₄(s)
4. PbSO₄(s) +Ag(s) $\to$ Ag⁺(aq) + Pb(s) +${\mathrm{SO}}_4^{2-}$ (aq)

The emf of the cell
Tl | Tl⁺ (0.001 M) || Cu²⁺ (1M) | Cu is 0.83V. The
emf of this cell could be increased by
1. Increasing in the concentration of Tl⁺ ions
2. Increasing in the concentration of Cu⁺ ions
3. Increasing in the concentration of both
4. None of the above

For a reaction A(s) + 2B⁺ $\to$ A²⁺ + 2B(s) ;  K_C has been found to be 10¹². The ${\mathrm{E}}_{\mathrm{cell}}^{°}$ is : 

The solution of nickel sulphate in which nickel
rod dipped is diluted to 10 times. The potential
of nickel
1. Decreases by 60 mV
2. Increases by 30 mV
3. Decreases by 30 mV
4. Decreases by 60 mV

Two electrodes are fitted in conductance cell
1.5cm apart while the area of cross-section of
each electrode is 0.75 cm². The cell constant is
1. 1.0125
2. 0.5cm
3. 2.0cm^–1
4. 0.2 cm^–1

Pick out the incorrect statement
1. Equivalent conductance increase with dilution
2. Molar conductance increase with dilution
3. Specific conductance increase with dilution
4. Specific resistance increase with dilution

In passing 3 faraday of electricity through the
three electrolytic cells connected in series
containing Ag⁺, Cu²⁺ and Al³⁺ respectively. The
molar ratio in which the three metal ions are
liberated at the electrode is
1. 1 : 2 : 3
2. 3 : 2 : 1
3. 6 : 3 : 2
4. 3 : 4 : 2

During electrolysis of fused calcium hydride, the
hydrogen is produced at
1. Cathode
2. Anode
3. Hydrogen is not liberated at all
4. H₂ produced reacts with oxygen to form water

The current liberates 0.504 g of hydrogen in 2
hours, the amount of copper liberated from a
solution of CuSO₄ by the same current flowing
for the same time would be
1. 31.8g
2. 63.6g
3. 15.9g
4. 6.36g

Given that
I₂ + 2e¯ $\to$ 2I¯; E° = 0.54V
Br₂ + 2e¯ $\to$ 2Br¯; E° = 1.09V
Predict which of the following is true?

The potential of hydrogen electrode having a
pH = 10 is
1. 0.59V
2. –0.59V
3. zero volts
4. –0.059V

What is the EMF of the cell?
Zn(s) | Zn⁺² (0.1M) || Sn⁺² (0.001M) | Sn(s)
Given ${\mathrm{E}}_{{\mathrm{Zn}}^{2+}/\mathrm{Zn}}^0=-0.76, {\mathrm{E}}_{{\mathrm{Sn}}^{2+}/\mathrm{Sn}}^0=-0.14 \mathrm{V}$
1. 0.62V
2. 0.56V
3. 1.12V
4. 0.31V

Zinc gives H₂ with H₂SO₄ and HCl but not with
HNO₃ because
1. Zinc acts as oxidising agent when reacts with
HNO₃
2. HNO₃ is a weaker acid then H₂SO₄ and HCl
3. In electrochemical series zinc is above
hydrogen
4. ${\mathrm{NO}}_3^{-}$ is reduced is preference to hydronium ion