Free Electrochemistry MCQs with Answers

• A. Hall's
• B. Nelson's
• C. Down's
• D. Hoope's

Explanation: The explanation for this question will be added soon.

• A. NaCl, NaClO, H2O
• B. NaCl , NaClO3 , H2O
• C. NaClO , NaClO3, H2O
• D. NaCl , H2O

Explanation: Cold dilute sodium hydroxide and chlorine gas reaction is disproportionation.

• A. Electroplating
• B. Conductivity
• C. Galvanizing
• D. Metallurgy

Explanation: In electroplating, we have the object replacing the cathode and the metal, the anode.

• A. Lead-acid accumulator
• B. H2 - O2 fuel cell
• C. Silver oxide battery
• D. Alkaline battery

Explanation: All the sources listed except H2 - O2 fuel cells produce electrical energy but they need to be disposed of eventually.

• A. Water
• B. HCI
• C. Na+
• D. NaCl

Explanation: In a diaphragm cell, which is a type of electrolytic cell used for the production of chlorine and sodium hydroxide, hydrogen gas is…

• A. (NH4)2Cr2O7
• B. K2Cr207
• C. Zn(CIO3)2
• D. KCIO3

Explanation: Equations for each reaction: A- (NH4)2Cr2O7 (aq) ⇌ N2 (g) + 4 H2O (l) + Cr2O3 (s) [No oxygen released] B- 4 K2Cr2O7(1) ⇌ 4K2CrO4(1) + 2…

• A. Graphite
• B. Copper
• C. Iron
• D. Silver

Explanation: The graphite anode has no reaction with chlorine, which is liberated at the anode.

• A. Free charge
• B. Electron
• C. Protons
• D. Zinc ions

Explanation: Option BCu+2 ions from the solution pick up the ELECTRONS at Cu electrode and get reduced to copper atoms ,hence Cu acts as a cathode and…

• A. Graphite
• B. Copper
• C. Iron
• D. Silver

Explanation: In a Down's cell, which is an electrolytic cell used for the production of sodium metal through the electrolysis of molten sodium chloride…

• A. Free electrons
• B. Positive ions
• C. Negative ions
• D. Both Options B and C are correct

Explanation: In electrolysis, current is carried through the electrolytic solution inside the cell by positive and negative ions using…

• A. Electrons
• B. Charges
• C. Energy
• D. Hydrogen ions

Explanation: Redox reactions (oxidation-reduction reactions) are actually the transfer of electrons.

• A. Sodium
• B. Hydrogen
• C. Chlorine
• D. Oxygen

Explanation: Chloride ions (Cl⁻) are attracted to the positive electrode (anode) during the electrolysis of a dilute solution of NaCl.

• A. Copper sulphate
• B. Copper chloride
• C. Zinc Chloride
• D. Zinc Sulphate

Explanation: Zinc, in a voltaic cell, is always dipped in zinc sulfate to get an excess of Zn2+ ions.

• A. (NH4)2Cr2O7
• B. K2Cr2O7
• C. Zn(ClO3)2
• D. KClO3

Explanation: This compound, also known as ammonium dichromate, decomposes upon heating to form chromium (lll) oxide, nitrogen gas, and water vapor.

• A. 10
• B. +1
• C. -1
• D. Zero

Explanation: The potential of the standard hydrogen electrode (SHE) is defined as 0 V under standard conditions.

• A. Emf(oxidation) - Emf(reduction)
• B. Emf(oxidation) + Emf(reduction)
• C. Emf(oxidation) x Emf(reduction)
• D. None of these options are correct

Explanation: This formula is present in the book:Emf of a cell = Oxidation Potential of Anode - Reduction Potential of Cathode.

• A. 2atm
• B. 780 mmHg
• C. 19 Psi
• D. 1 atm

Explanation: To setup a standard half-cell, the conditions are 298.15 Kelvin (temperature), 1 atmosphere (pressure), and have a Molarity of 1.0 M for…

• A. Nitrous oxide
• B. Nitric oxide
• C. Nitrogen peroxide
• D. Nitrous anhydride

Explanation: Nitric oxide =+2Nitrous oxide = +1Nitrous anhydride= +3Nitrogen peroxide= +5

• A. ±2
• B. +4 and +6
• C. None of these
• D. Both A and B

Explanation: In H₂SO₄, the oxidation number of S is +6.In H₂SO₃, the oxidation number of S is +4.In Na₂S₂O₃, the oxidation number of S is +2.

• A. Redox Potential
• B. Oxidation Potential
• C. EMF of the cell
• D. Reduction Potential

Explanation: A stronger oxidizing agent means it undergoes reduction more easily and thus has greater standard reduction potential.