Electro chemistry practice · Easy

Option A (Oxidation occur at onode in both galvanic and electrolytic cell) is correct because oxidation always occurs at the anode, regardless of whether it's a galvanic or electrolytic cell.

Option B (271.44) is correct because it is calculated using Kohlrausch's law of independent migration of ions.

Option A (Anode) is correct because zinc has a higher oxidation potential than hydrogen, so it will be oxidized at the anode.

The correct answer is B ($\mathrm{S}{\kern 1pt} {\kern 1pt} {\mathrm{m}^2}{\kern 1pt} {\kern 1pt}\mathrm{mo}{\mathrm{l}^{ - 1}}$) because it represents the units of molar conductivity, which is the constant of proportionality in the given relationship.

Option B (Zinc container) is correct because in a Leclanche cell (dry cell), the zinc container acts as the anode (negative electrode) where oxidation occurs.

Option D (All of the above) is correct because solute-solute interactions, solute-solvent interactions, and temperature all influence the conductance of a solution.

Option D is correct because a spontaneous electrochemical cell has a negative Gibbs free energy change and a positive standard cell potential.

Option B ($\mathrm{c}{\mathrm{m}^{ - 1}}$) is correct because cell constant is defined as the ratio of length to area, resulting in units of inverse length.

Option B ($\mathrm{oh}{\mathrm{m}^{ - 1}}{\kern 1pt} {\kern 1pt}\mathrm{c}{\mathrm{m}^{ - 1}}{\kern 1pt} {\kern 1pt}{\rm{or {\kern 1pt} {\kern 1pt}S}}{\kern 1pt} {\kern 1pt}{\mathrm{m}^{ - 1}}$) is the correct SI unit of conductivity, which is Siemens per meter (S/m) or ohm$^{-1}$m$^{-1}$.

Option B is correct because Pb is above Ag but below Ni in the electrochemical series, meaning it can reduce $\mathrm{A}{\mathrm{g}^ + }$ but not $\mathrm{N}{\mathrm{i}^{2 + }}$.

Option C (2 F) is correct because the production of one mole of copper from copper sulfate requires two moles of electrons, which corresponds to 2 Faradays of electricity.

The correct answer is B ($KCl > NaCl > LiCl$) because the equivalent conductivity at infinite dilution depends on the ionic mobility, which is inversely related to the hydrated ionic size. Smaller ions are more heavily hydrated, reducing their mobility.

Option B (Reference electrode) is correct because the calomel electrode is a well-defined half-cell with a known and stable potential, making it suitable as a reference for electrochemical measurements.