MHT CET 2023 13th May Morning Shift | Electrochemistry Question 56 | Chemistry

Calculate the time required in second to deposit $$6.35 \mathrm{~g}$$ copper from its salt solution by passing 5 ampere current. [Molar mass of $$\mathrm{Cu}=63.5 \mathrm{~g} \mathrm{~mol}^{-1}$$ ]

3600

3700

3860

4000

MHT CET 2023 12th May Evening Shift

MCQ (Single Correct Answer)

-0

Which of the following expressions represents molar conductivity of $$\mathrm{AB}_3$$ type electrolyte?

$$3 \lambda_{\mathrm{A}^{\cdots}}^{\circ}+\lambda_{\mathrm{B}^{-}}^{\circ}$$

$$\lambda_{\mathrm{A}^{\cdots}}^{\circ}+\lambda_{\mathrm{B}^{-}}^{\circ}$$

$$\lambda_{\mathrm{A}^{\cdots}}^{\circ}+3\lambda_{\mathrm{B}^{-}}^{\circ}$$

$$2\lambda_{\mathrm{A}^{\cdots}}^{\circ}+\lambda_{\mathrm{B}^{-}}^{\circ}$$

MHT CET 2023 12th May Evening Shift

MCQ (Single Correct Answer)

-0

Calculate the $$\mathrm{E}_{\text {cell }}$$ for $$\mathrm{Zn}_{(\mathrm{s})}\left|\mathrm{Zn}_{(0.1 \mathrm{M})}^{++}\right|\left|\mathrm{Cr}_{(0.1 \mathrm{M})}^{+++}\right| \mathrm{Cr}_{(\mathrm{s})}$$ at $$25^{\circ} \mathrm{C}$$ if $$\mathrm{E}_{\text {cell }}^{\circ}$$ is $$0.02 \mathrm{~V}$$

$$-0.05 \mathrm{~V}$$

$$0.03 \mathrm{~V}$$

$$-0.06 \mathrm{~V}$$

$$0.07 \mathrm{~V}$$

MHT CET 2023 12th May Evening Shift

MCQ (Single Correct Answer)

-0

A conductivity cell containing $$5 \times 10^{-4} \mathrm{~M} \mathrm{~NaCl}$$ solution develops resistance $$14000 \mathrm{~ohms}$$ at $$25^{\circ} \mathrm{C}$$. Calculate the conductivity of solution if the cell constant is $$0.84 \mathrm{~cm}^{-1}$$

$$6.0 \times 10^{-5} \Omega^{-1} \mathrm{~cm}^{-1}$$

$$3.0 \times 10^{-5} \Omega^{-1} \mathrm{~cm}^{-1}$$

$$9.0 \times 10^{-5} \Omega^{-1} \mathrm{~cm}^{-1}$$

$$12.0 \times 10^{-5} \Omega^{-1} \mathrm{~cm}^{-1}$$

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