The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9S cm 2 mol -1 . Calculate the conductivity of the conductivity of this solution. - Wired Faculty

Electrochemistry

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The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9S cm²mol^-1. Calculate the conductivity of the conductivity of this solution.

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Molar space conductivity comma space straight k equals space conductivity over Concentration straight capital lambda subscript straight m space equals straight k over straight c conductivity comma straight k equals space straight capital lambda subscript straight m space equals straight k over straight c conductivity comma space straight k equals space straight capital lambda subscript straight m space straight x space straight C equals space fraction numerator 138.9 space left parenthesis Scm squared space mol to the power of negative 1 end exponent right parenthesis space straight x space 1.5 space left parenthesis mol divided by straight L right parenthesis over denominator 1000 space left parenthesis cm cubed divided by straight L right parenthesis end fraction space equals 0.208 space straight S space cm to the power of negative 1 end exponent

Some More Questions From Electrochemistry Chapter

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°_m value of water.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

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Electrochemistry

The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9S cm²mol^-1. Calculate the conductivity of the conductivity of this solution.

Some More Questions From Electrochemistry Chapter

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°_m value of water.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

Suggest a list of metals that are extracted electrolytically.

Consider the reaction: Cr₂O₇^2– + 14H⁺ + 6e- → 2Cr³⁺ + 8H₂O
What is the quantity of electricity in coulombs needed to reduce 1 mol of Cr₂O₇^2-?

Write the chemistry of recharging the lead storage battery, highlighting all the materials that are involved during recharging.

Suggest two materials other than hydrogen that can be used as fuels in fuel cells.

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Electrochemistry

The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9S cm2mol-1. Calculate the conductivity of the conductivity of this solution.

Some More Questions From Electrochemistry Chapter

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°m value of water.

The molar conductivity of 0.025 mol L–1 methanoic acid is 46.1 S cm2 mol–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H+) = 349.6 S cm2 mol–1 and λ° (HCOO– ) = 54.6 s cm2 mol–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

Suggest a list of metals that are extracted electrolytically.

Consider the reaction: Cr2O72– + 14H+ + 6e- → 2Cr3+ + 8H2OWhat is the quantity of electricity in coulombs needed to reduce 1 mol of Cr2O72-?

Write the chemistry of recharging the lead storage battery, highlighting all the materials that are involved during recharging.

Suggest two materials other than hydrogen that can be used as fuels in fuel cells.

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation

The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9S cm²mol^-1. Calculate the conductivity of the conductivity of this solution.

Suggest a way to determine the Λ°_m value of water.

The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

Consider the reaction: Cr₂O₇^2– + 14H⁺ + 6e- → 2Cr³⁺ + 8H₂O
What is the quantity of electricity in coulombs needed to reduce 1 mol of Cr₂O₇^2-?