MCQOPTIONS
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MCQOPTIONS
This section includes 12 Mcqs, each offering curated multiple-choice questions to sharpen your Chemistry knowledge and support exam preparation. Choose a topic below to get started.
| 1. |
Find the number of electrons transferred in the equation Cu(g) + 2Ag+(aq) Cu2+(aq) + 2Ag(s). |
| A. | 4 |
| B. | 3 |
| C. | 2 |
| D. | 1 |
| Answer» D. 1 | |
| 2. |
What is the number of electrons transferred in an equation if the Nernst equation is E(cell) = E (cell) 9.83 10-3 log10 (Anode / Cathode)? |
| A. | 2 |
| B. | 6 |
| C. | 4 |
| D. | 1 |
| Answer» C. 4 | |
| 3. |
What is the value of universal gas constant in Nernst equation when the potential is given in volts? |
| A. | 8.314 J mol<sup>-1</sup>K<sup>-1</sup> |
| B. | 0.0821 L atm mol<sup>-1</sup>K<sup>-1</sup> |
| C. | 8.205 m<sup>3</sup> atm mol<sup>-1</sup>K<sup>-1</sup> |
| D. | 1.987 cal mol<sup>-1</sup>K<sup>-1</sup> |
| Answer» B. 0.0821 L atm mol<sup>-1</sup>K<sup>-1</sup> | |
| 4. |
What is the pH of HCl solution when the hydrogen gas electrode shows a potential of -0.22 V at standard temperature and pressure? |
| A. | 2.17 |
| B. | 2.98 |
| C. | 3.73 |
| D. | 3.14 |
| Answer» D. 3.14 | |
| 5. |
A zinc rod dipped in n molar solution of ZnSO4 has an electrode potential of -0.56 V. The salt is 98 percent dissociated at room temperature. What is the molarity of the solution? (E (Zn+2/Zn) = -0.5 V) |
| A. | 8.44 10<sup>-3</sup> M |
| B. | 9.44 10<sup>-4</sup> M |
| C. | 8.44 10<sup>-4</sup> M |
| D. | 9.44 10<sup>-3</sup> M |
| Answer» E. | |
| 6. |
Calculate the electrode potential of the given electrode.
|
| A. | 3.51 V |
| B. | 3.55 V |
| C. | 1.26 V |
| D. | 2.95 V |
| Answer» B. 3.55 V | |
| 7. |
The e.m.f and the standard e.m.f of a cell in the following reaction is 5 V and 5.06 V at room temperature, Ni(s) + 2Ag+(n) Ni2+(0.02M) + 2Ag(s). What is the concentration of Ag+ ions? |
| A. | 0.0125 M |
| B. | 0.0314 M |
| C. | 0.0625 M |
| D. | 0.0174 M |
| Answer» E. | |
| 8. |
What is the correct Nernst equation for M2+ (aq) + 2e+ M (s) at 45 C? |
| A. | E <sub>(M2+/M)</sub> + 0.315log<sub>10</sub> (1 / [M]<sup>+2</sup>) |
| B. | E <sub>(M2+/M)</sub> + 0.0425log<sub>10</sub> (1 / [M]<sup>+2</sup>) |
| C. | E <sub>(M2+/M)</sub> + 0.0315log<sub>10</sub> (1 / [M]<sup>+2</sup>) |
| D. | E <sub>(M2+/M)</sub> + 0.0326log<sub>10</sub> (1 / [M]<sup>+2</sup>) |
| Answer» D. E <sub>(M2+/M)</sub> + 0.0326log<sub>10</sub> (1 / [M]<sup>+2</sup>) | |
| 9. |
The equilibrium constant for a cell reaction, Cu(g) + 2Ag+(aq) Cu2+(aq) + 2Ag (s) is 4 1016. Find E (cell) for the cell reaction. |
| A. | 0.63 V |
| B. | 0.49 V |
| C. | 1.23 V |
| D. | 3.24 V |
| Answer» C. 1.23 V | |
| 10. |
Calculate the e.m.f. of the half-cell given below.
|
| A. | 4 V |
| B. | 5.6 V |
| C. | 3.4 V |
| D. | 5.4 V |
| Answer» E. | |
| 11. |
Calculate the equilibrium constant for the reaction Fe + CuSO4 FeSO4 + Cu at 25 C.
|
| A. | 3.46 10<sup>30</sup> |
| B. | 3.46 10<sup>26</sup> |
| C. | 3.22 10<sup>30</sup> |
| D. | 3.22 10<sup>26</sup> |
| Answer» D. 3.22 10<sup>26</sup> | |
| 12. |
The standard oxidation potential of Ni/Ni2+ electrode is 0.3 V. If this is combined with a hydrogen electrode in acid solution, at what pH of the solution with the measured e.m.f. be zero at 25 C? (Assume [Ni2+] = 1M) |
| A. | 5.08 |
| B. | 4 |
| C. | 4.5 |
| D. | 5.25 |
| Answer» B. 4 | |