MHT-CET Electrochemistry — practice questions
30 free MCQs with worked solutions. Tap any question for the answer + explanation, or practice them all in the app.
Practice MHT-CET Electrochemistry in the app →A substance whose aqueous solution conducts electricity by dissociation into ions is called a(n):The SI unit of electrical conductance is:**Conductivity** $\kappa$ of a solution refers to:**Molar conductivity** $\Lambda$ is defined as:**Kohlrausch's law** of independent migration of ions states that at infinite dilution:On dilution, the **conductivity** ($\kappa$) of an electrolyte solution:On dilution, the **molar conductivity** ($\Lambda$) of an electrolyte:The **degree of dissociation** $\alpha$ of a weak electrolyte is related to its molar conductivity by:**Cell constant** of a conductivity cell is given by:For a **strong** electrolyte (e.g. KCl), the variation of molar conductivity $\Lambda$ with $ qrt{c}$ is:The molar conductivity of 0.05 M BaCl₂ solution at 25 °C is 223 Ω⁻¹ cm² mol⁻¹. Its conductivity ($\kappa$) is:Using Kohlrausch's law, if $\Lambda_0$(NaI) = 126.9, $\Lambda_0$(AgNO₃) = 133.4, $\Lambda_0$(NaNO₃) = 121.5 (aGiven molar ionic conductivities $\lambda^0$: Ca²⁺ = 104, Cl⁻ = 76.4 (Ω⁻¹ cm² mol⁻¹), the molar conductivity aThe molar conductivity of 0.01 M acetic acid is 16.5 Ω⁻¹ cm² mol⁻¹, and $\Lambda_0$ = 390.7 Ω⁻¹ cm² mol⁻¹. TheA conductivity cell containing 0.01 M KCl ($\kappa = 0.00141$ Ω⁻¹ cm⁻¹) at 25 °C has resistance 604 Ω. The celFor weak electrolytes, why is $\Lambda_0$ determined indirectly (via Kohlrausch's law from strong electrolyte In a galvanic cell, the **anode** is the electrode at which:In a galvanic cell, current in the external circuit flows from:The Gibbs free-energy change of a galvanic cell reaction is given by:For a cell with $E^0 = 1.10$ V and $n = 2$ electrons transferred, the standard Gibbs energy change $\Delta G^0Which of the following is the correct **decreasing order** of standard reduction potential (i.e. from strongesA salt bridge in a galvanic cell:A conductivity cell has cell constant 0.852 cm⁻¹. Filled with 0.001 M AgNO₃ solution, it shows resistance 6530For 0.01 M acetic acid at 25 °C, $\Lambda_c = 16.5$ Ω⁻¹ cm² mol⁻¹ and $\Lambda_0 = 390.7$ Ω⁻¹ cm² mol⁻¹. The dThe molar conductivities of HCl, CH₃COONa, and NaCl at infinite dilution are 426.1, 91.0 and 126.4 Ω⁻¹ cm² molFor the cell Zn|Zn²⁺‖Cu²⁺|Cu with $E^0_{cell} = 1.10$ V, the equilibrium constant $K$ at 298 K ($n=2$, RT/F = The **Nernst equation** for a half-cell reaction (M^n+ + n e⁻ → M) at 298 K can be written as:A current of 2 A is passed through molten CuCl₂ for 30 minutes. The mass of copper deposited at the cathode isFor a galvanic cell, $\Delta G^0$ of the cell reaction is −58 kJ/mol, with $n = 2$ electrons transferred. The Two electrolytic cells, one with AgNO₃ and another with CuSO₄, are connected in **series** and the same curren