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Electrochemistry formulas

Master Electrochemistry through 22 JEE Advanced-level formulas, systematically structured with every variable spelled out. Revise concept-wise, identify the areas where you need improvement, and focus your preparation with greater precision.

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Electrochemistry, every formula

22 formulas, typeset and free. Print it, or keep it open beside your practice.

Standard cell potential
$E_{ce l l}^{\circ} = E_{c a t h o d e}^{\circ} - E_{an o d e}^{\circ}$
Nernst equation
$E = E^{\circ} - \frac{0.0591}{n} lo g Q (2 5^{\circ} C)$
Q1MCQNernst
The Nernst equation at $25^{\circ}$C is:
- A
  $E=E^{\circ}-\dfrac{0.0591}{n}\log Q$
- B
  $E=E^{\circ}+\dfrac{0.0591}{n}\log Q$
- C
  $E=E^{\circ}-nFQ$
- D
  $E=E^{\circ}$
Nernst (general)
$E = E^{\circ} - \frac{R T}{n F} ln Q$
Q1MCQNernst general
The general Nernst equation is:
- A
  $E=E^{\circ}-\dfrac{RT}{nF}\ln Q$
- B
  $E=E^{\circ}-nF\ln Q$
- C
  $E=E^{\circ}RT$
- D
  $E=nF$
ΔG and cell potential
$Δ G = - n F E_{ce l l}$
Q1MCQΔG and E
The Gibbs energy of a cell reaction is:
- A
  $-nFE_{cell}$
- B
  $nFE_{cell}$
- C
  $-\dfrac{E_{cell}}{nF}$
- D
  $FE_{cell}$
ΔG° and E°
$Δ G^{\circ} = - n F E_{ce l l}^{\circ}$
Q1MCQΔG° and E°
The standard Gibbs energy is:
- A
  $-nFE^{\circ}_{cell}$
- B
  $nFE^{\circ}_{cell}$
- C
  $-FE^{\circ}$
- D
  $0$
E° and equilibrium constant
$E^{\circ} = \frac{0.0591}{n} lo g K$
Q1MCQE° and K
The relation between $E^{\circ}$ and $K$ is:
- A
  $E^{\circ}=\dfrac{0.0591}{n}\log K$
- B
  $E^{\circ}=-\dfrac{0.0591}{n}\log K$
- C
  $E^{\circ}=nK$
- D
  $E^{\circ}=\log K$
Faraday's first law
$m = \frac{Z I t}{1} = \frac{M I t}{n F}$
Q1MCQFaraday's law
The mass deposited during electrolysis is:
- A
  $\dfrac{M\,It}{nF}$
- B
  $\dfrac{nF}{M\,It}$
- C
  $M\,It$
- D
  $\dfrac{It}{M}$
Charge
$Q = I t$
Faraday constant
$F = 96500 C/mol$
Q1MCQFaraday constant
The value of the Faraday constant is:
- A
  $96500$ C/mol
- B
  $6.022\times10^{23}$
- C
  $8.314$
- D
  $1.6\times10^{-19}$
Equivalents deposited
$equivalents = \frac{I t}{F}$
Conductance
$G = \frac{1}{R}$
Q1MCQConductance
Conductance is:
- A
  $\dfrac{1}{R}$
- B
  $R$
- C
  $R^{2}$
- D
  $\dfrac{R}{2}$
Specific conductance (conductivity)
$κ = \frac{1}{R} \cdot \frac{l}{A} = G \cdot \frac{l}{A}$
Q1MCQConductivity
The specific conductance (conductivity) is:
- A
  $G\cdot\dfrac{l}{A}$
- B
  $\dfrac{G}{l/A}$
- C
  $GA$
- D
  $\dfrac{1}{G}$
Cell constant
$\frac{l}{A} = R κ$
Q1MCQCell constant
The cell constant is:
- A
  $\dfrac{l}{A}$
- B
  $\dfrac{A}{l}$
- C
  $lA$
- D
  $\dfrac{1}{lA}$
Molar conductivity
$Λ_{m} = \frac{κ \times 1000}{C}$
Q1MCQMolar conductivity
The molar conductivity is:
- A
  $\dfrac{\kappa\times1000}{C}$
- B
  $\dfrac{C}{\kappa}$
- C
  $\kappa C$
- D
  $\dfrac{\kappa}{1000C}$
Kohlrausch's law
$Λ_{m}^{\circ} = λ_{+}^{\circ} + λ_{-}^{\circ}$
Q1MCQKohlrausch
Kohlrausch's law states the limiting molar conductivity is:
- A
  $\lambda_+^{\circ}+\lambda_-^{\circ}$
- B
  $\lambda_+^{\circ}\lambda_-^{\circ}$
- C
  $\lambda_+^{\circ}-\lambda_-^{\circ}$
- D
  $\dfrac{\lambda_+^{\circ}}{\lambda_-^{\circ}}$
Degree of dissociation
$α = \frac{Λ _{m}}{Λ _{m}^{\circ}}$
Q1MCQDegree of dissociation
The degree of dissociation of a weak electrolyte is:
- A
  $\dfrac{\Lambda_m}{\Lambda_m^{\circ}}$
- B
  $\dfrac{\Lambda_m^{\circ}}{\Lambda_m}$
- C
  $\Lambda_m\Lambda_m^{\circ}$
- D
  $\Lambda_m^{\circ}-\Lambda_m$
Dissociation constant (weak)
$K_{a} = \frac{C α ^{2}}{1 - α}$
Q1MCQKa (conductivity)
The dissociation constant of a weak acid is:
- A
  $\dfrac{C\alpha^{2}}{1-\alpha}$
- B
  $C\alpha$
- C
  $\dfrac{\alpha}{C}$
- D
  $C\alpha^{2}$
EMF and spontaneity
$E_{ce l l} > 0 \Rightarrow spontaneous$
Q1MCQEMF spontaneity
A cell reaction is spontaneous when:
- A
  $E_{cell}>0$
- B
  $E_{cell}<0$
- C
  $E_{cell}=0$
- D
  $\Delta G>0$
Concentration cell EMF
$E = \frac{0.0591}{n} lo g \frac{C _{2}}{C _{1}}$
Q1MCQConcentration cell
The EMF of a concentration cell is:
- A
  $\dfrac{0.0591}{n}\log\dfrac{C_2}{C_1}$
- B
  $\dfrac{0.0591}{n}\log(C_1 C_2)$
- C
  $E^{\circ}$
- D
  $0$
Standard hydrogen electrode
$E_{S H E}^{\circ} = 0 V$
Molar conductivity units
$S cm^{2} mol^{- 1}$
Q1MCQΛm units
The units of molar conductivity are:
- A
  S cm$^{2}$ mol$^{-1}$
- B
  S cm$^{-1}$
- C
  $\Omega$ cm
- D
  C mol$^{-1}$
Weight from equivalent
$m = \frac{E I t}{F}$
E = equivalent weight
Q1MCQWeight from equivalent
The mass deposited using equivalent weight $E$ is:
- A
  $\dfrac{E\,It}{F}$
- B
  $\dfrac{F}{E\,It}$
- C
  $E\,It$
- D
  $\dfrac{It}{E}$

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Electrochemistry formulas

Electrochemistry, every formula

Standard cell potential

Nernst equation

Nernst (general)

ΔG and cell potential

ΔG° and E°

E° and equilibrium constant

Faraday's first law

Charge

Faraday constant

Equivalents deposited

Conductance

Specific conductance (conductivity)

Cell constant

Molar conductivity

Kohlrausch's law

Degree of dissociation

Dissociation constant (weak)

EMF and spontaneity

Concentration cell EMF

Standard hydrogen electrode

Molar conductivity units

Weight from equivalent

More JEE Advanced Chemistry formula sheets

Other ways to revise this chapter

Preparing students for India’s top institutes

Join QuestPix, Today!