Equilibrium Constant from Nernst Equation
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Q.
The standard electrode potentials of Zn2+Zn and Ag+Ag are −0.763 V and +0.799 V respectively. The standard potential of the cell is
1.562 V
2.361 V
−1.562 V
−2.361 V
Q. E∘ for the cell is Zn |Zn2+ (aq)||Cu2+ (aq)| Cu at 25∘C, the equilibrium constant for the reaction Zn+Cu2+(aq)⇌Cu+Zn2+ (aq) is of the order of
- 10−37
- 10−28
- 10+18
- 10+17
Q. EMF of the cell, Ag|AgNO3(0.1M)|KBr(1N), AgBr(s)|Ag is −0.6 V at 298 K
Calculate the Ksp of AgBr at 298 K.
Calculate the Ksp of AgBr at 298 K.
- Ksp=4.0×10−12
- Ksp=3.5×10−12
- Ksp=4.8×10−12
- Ksp=3.8×10−12
Q.
Electra needs to answer this question to master this topic.
Help her calculate the equilibrium constant of the following reaction:
Cu(s)+2Ag+(aq)→Cu2+(aq)+2Ag(s)
E0cell=0.46V
The options below are logK values where K is the equilibrium constant.
15.45
- 15.59
- 15.93
- 19.5
Q. The equilibrium constant for the following reaction is 1030. Calculate E∘ (in volts) for the cell at 298 K.
2X2(s)+3Y2+(aq)→2X3+2(aq)+3Y(s)
2X2(s)+3Y2+(aq)→2X3+2(aq)+3Y(s)
- +0.105 V
- +0.295 V
- +0.0985 V
- -0.295 V
Q. E∘ for the cell is Zn |Zn2+ (aq)||Cu2+ (aq)| Cu at 25∘C, the equilibrium constant for the reaction Zn+Cu2+(aq)⇌Cu+Zn2+ (aq) is of the order of
- 10−37
- 10−28
- 10+18
- 10+17
Q. If the E0cell for a given reaction has a negative value, which of the following gives the correct relationships for the values of ΔG0 and Keq ?
- ΔG∘>0;Keq<1
- ΔG∘>0;Keq>1
- ΔG∘<0;Keq>1
- ΔG∘<0;Keq<1
Q. For a cell involving one electron, E0cell = 0.59 V at 298 K, the equilibrium constant for the cell reaction is:
[Given that 2.303RTF = 0.059 V at T = 298 K]
[Given that 2.303RTF = 0.059 V at T = 298 K]
- 1.0×102
- 1.0×105
- 1.0×1010
- 1.0×1030
Q. In a cell that utilizes the reaction Zn(s)+2H+(aq)→Zn2+(aq)+H2 (g) addition of H2SO4 to cathode compartment, will
- Increase the E and shift equilibrium to the right
- Lower the E and shift equilibrium to the right
- Lower the E and shift equilibrium to the left
- Increase the E and shift equilibrium to the left
Q. In a cell that utilizes the reaction Zn(s)+2H+(aq)→Zn2+(aq)+H2 (g) addition of H2SO4 to cathode compartment, will
- Increase the E and shift equilibrium to the right
- Lower the E and shift equilibrium to the right
- Lower the E and shift equilibrium to the left
- Increase the E and shift equilibrium to the left