#cell constant

CHEMISTRY

What is the ll constant if the resistance of a conductivity ll with 0.01 M KCl solution is 200 Ω and its conductivity i

Given: What is the ll constant if the resistance of a conductivity ll with 0.01 M KCl solution is 200 Ω and its conductivity is 0.14 × 10⁻² S cm⁻¹? These values define the system as per NCERT data. Formula: Cell constant, G^* = kappa × R = 0.14 × 10⁻² × 200 = 0.28 cm^{-1 .. This is the standard NCERT relation for this phenomenon. Substitution & Calculation: Substituting values like 1.2 × 10⁻⁵, 236 J kg⁻¹ K⁻¹, CH₃CH₂NH₂ etc. into the formula and simplifying step by step. Result: The computed value matches the expected outcome and confirms the correct choice. Units and powers like J kg⁻¹ K⁻¹, m/s², 10⁻⁵ are properly used as per NCERT.

Ref: NCERT Chemistry Textbook for Class XI and XII, Chapter: Solutions, Topic: Concentration terms and colligative properties.

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Nernst Equation and Gibbs Energy and Equilibrium Constant

The resistance of a conductivity cell with 0.01 M NaCl solution is 250 Ω, and its conductivity is 0.0012 S cm⁻¹. What is

kappa = (cell constant/R) , 0.0012 = (cell constant/250) , cell constant = 0.3 cm⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

What is the cell constant of a conductivity cell if the resistance of a 0.01 M KCl solution is 200 Ω and its conductivit

kappa = (cell constant/R) , 0.00141 = (cell constant/200) , cell constant = 0.282 cm⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

What is the cell constant if the resistance of a 0.05 M KCl solution is 100 Ω and its conductivity is 0.0065 S cm⁻¹?

kappa = (cell constant/R) , 0.0065 = (cell constant/100) , cell constant = 0.65 cm⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Nernst Equation and Gibbs Energy and Equilibrium Constant

The resistance of a conductivity cell with 0.001 M KCl solution is 1500 Ω, and its conductivity is 0.146 × 10⁻³ S cm⁻¹.

kappa = (cell constant/R) , 0.146 × 10⁻³ = (cell constant/1500) , cell constant = 0.219 cm⁻¹.

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant

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Electrolytic Cells and Electrolysis and Faraday's Laws

The resistance of a conductivity cell with 0.02 M NaCl solution is 500 Ω, and its conductivity is 0.0024 S cm⁻¹. What is

kappa = (cell constant/R) , 0.0024 = (cell constant/500) , cell constant = 1.2 cm⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrolytic Cells and Electrolysis and Faraday's Laws

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Electrochemical Cells - Galvanic Cells and Electrode Potential

The resistance of a conductivity cell with 0.02 M KCl solution is 400 Ω, and its conductivity is 0.0025 S cm⁻¹. What is

kappa = (cell constant/R) , 0.0025 = (cell constant/400) , cell constant = 1.0 cm⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Electrochemical Cells - Galvanic Cells and Electrode Potential

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Conductance - Conductivity Molar Conductivity and Kohlrausch Law

A conductivity cell with cell constant 0.6 cm⁻¹ shows a resistance of 200 Ω with a 0.03 M KCl solution. What is the mola

kappa = (cell constant/R) = (0.6/200) = 0.003 S cm⁻¹ . Lambdam = (kappa × 1000/c) = (0.003 × 1000/0.03) = 100 S cm² mol⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Conductance - Conductivity Molar Conductivity and Kohlrausch Law

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Conductance - Conductivity Molar Conductivity and Kohlrausch Law

A conductivity cell with cell constant 0.6 cm⁻¹ shows a resistance of 200 Ω with a 0.03 M KCl solution. What is the mola

kappa = (cell constant/R) = (0.6/200) = 0.003 S cm⁻¹ . Lambdam = (kappa × 1000/c) = (0.003 × 1000/0.03) = 100 S cm² mol⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Conductance - Conductivity Molar Conductivity and Kohlrausch Law

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Conductance - Conductivity Molar Conductivity and Kohlrausch Law

A conductivity cell with cell constant 0.5 cm⁻¹ shows a resistance of 200 Ω with a 0.02 M KCl solution. What is the mola

kappa = (cell constant/R) = (0.5/200) = 0.0025 S cm⁻¹ . Lambdam = (kappa × 1000/c) = (0.0025 × 1000/0.02) = 125 S cm² mol⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Conductance - Conductivity Molar Conductivity and Kohlrausch Law

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Conductance - Conductivity Molar Conductivity and Kohlrausch Law

A conductivity cell with cell constant 0.5 cm⁻¹ shows a resistance of 200 Ω with a 0.02 M KCl solution. What is the mola

kappa = (cell constant/R) = (0.5/200) = 0.0025 S cm⁻¹ . Lambdam = (kappa × 1000/c) = (0.0025 × 1000/0.02) = 125 S cm² mol⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Conductance - Conductivity Molar Conductivity and Kohlrausch Law

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Conductance - Conductivity Molar Conductivity and Kohlrausch Law

A conductivity cell with cell constant 0.4 cm⁻¹ shows a resistance of 250 Ω with a 0.02 M NaCl solution. What is the mol

kappa = (cell constant/R) = (0.4/250) = 0.0016 S cm⁻¹ . Lambdam = (kappa × 1000/c) = (0.0016 × 1000/0.02) = 80 S cm² mol⁻¹ .

Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Conductance - Conductivity Molar Conductivity and Kohlrausch Law

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