Ques 1. Calculate the standard EMF of a cell which involves the following cell reaction:
$\ce{ Zn + 2 Ag^+ -> Zn^{2+} + 2 Ag}$
Given that $\ce{ {E^0}_{Zn^{2+}/Zn} = -0.76 volt }$ and
$\ce{ {E^0}_{Ag^+/Ag} = 0.80 volt }$
Ques 2. Calculate the standard EMF of the cell, containing Zinc and Nickel electrodes.
Given that $\ce{ {E^0}_{Zn^{2+}/Zn} = -0.76 volt }$ and
$\ce{ {E^0}_{Ni^{2+}/Ni} = -0.25 volt }$
Ques 3. For th cell show below:
$\ce{ Zn (s) \mid ZnSO4 (aq) \mid \mid CuSO4 (aq) \mid Cu (s) }$
calculate standard cell potential if standard state reduction potentials for $\ce{ Cu^{2+}/Cu \, and \, Zn^{2+}/Zn }$ are 0.34 V and - 0.76 V respectively.
Ques 4. Two half-cells in a galvanic cell are \( Al^{3+}(aq) \mid Al \, and \, Mg^{2+} (aq) \mid Mg \). Given that the reduction potentials of the half-cells are - 1.66 V and - 2.36 V respectively. Calculate the cell potential.
Ques 5. For the galvanic cell $\ce{ Zn \mid Zn^{2+}(1M) \mid \mid Ag^+(1M) \mid Ag }$ calculate the cell potential when the standard reduction potentials of Zn and Ag electrodes are - 0.763 V and + 0.80 V respectively.
Ques 6. The emf \( (E^0) \) of the following cell are:
$\ce{ Ag \mid Ag^+(1M) \mid \mid Cu^{2+}(1M) \mid Cu; \,E^0 = - 0.46 V}$ and
$\ce{ Zn \mid Zn^{2+}(1M) \mid \mid Cu^{2+}(1M) \mid Cu; \,E^0 = + 1.10 V}$
Calculate the emf of the cell
$\ce{ Zn \mid Zn^{2+}(1M) \mid \mid Ag^+(1M) \mid Ag }$
Ques 7. An electrochemical cell is made up of copper and silver electrodes with their standard reduction potentials 0.34 V and 0.80 V respectively. Select the anode and cathode, represent the cell and write the cell reaction. Find the emf of cell.
$\ce{ {E^0}_{Ag^+/Ag} = 0.80 volt }$
Ques 2. Calculate the standard EMF of the cell, containing Zinc and Nickel electrodes.
Given that $\ce{ {E^0}_{Zn^{2+}/Zn} = -0.76 volt }$ and
$\ce{ {E^0}_{Ni^{2+}/Ni} = -0.25 volt }$
Ques 3. For th cell show below:
$\ce{ Zn (s) \mid ZnSO4 (aq) \mid \mid CuSO4 (aq) \mid Cu (s) }$
calculate standard cell potential if standard state reduction potentials for $\ce{ Cu^{2+}/Cu \, and \, Zn^{2+}/Zn }$ are 0.34 V and - 0.76 V respectively.
Ques 4. Two half-cells in a galvanic cell are \( Al^{3+}(aq) \mid Al \, and \, Mg^{2+} (aq) \mid Mg \). Given that the reduction potentials of the half-cells are - 1.66 V and - 2.36 V respectively. Calculate the cell potential.
Ques 5. For the galvanic cell $\ce{ Zn \mid Zn^{2+}(1M) \mid \mid Ag^+(1M) \mid Ag }$ calculate the cell potential when the standard reduction potentials of Zn and Ag electrodes are - 0.763 V and + 0.80 V respectively.
Ques 6. The emf \( (E^0) \) of the following cell are:
$\ce{ Ag \mid Ag^+(1M) \mid \mid Cu^{2+}(1M) \mid Cu; \,E^0 = - 0.46 V}$ and
$\ce{ Zn \mid Zn^{2+}(1M) \mid \mid Cu^{2+}(1M) \mid Cu; \,E^0 = + 1.10 V}$
Calculate the emf of the cell
$\ce{ Zn \mid Zn^{2+}(1M) \mid \mid Ag^+(1M) \mid Ag }$
Ques 7. An electrochemical cell is made up of copper and silver electrodes with their standard reduction potentials 0.34 V and 0.80 V respectively. Select the anode and cathode, represent the cell and write the cell reaction. Find the emf of cell.