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JEE Advanced: Gas Laws, Solutions and Electrochemistry

Flashcards on gas laws, colligative properties, kinetics, equilibrium and electrochemistry for JEE Advanced. Original study material.

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Boyle's law

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Boyle's law

P_{1} V_{1} = P_{2} V_{2}

at constant temperature.

Charles's law

\frac{V _{1}}{T _{1}} = \frac{V _{2}}{T _{2}}

at constant pressure, T in kelvin.

Combined gas law

\frac{P _{1} V _{1}}{T _{1}} = \frac{P _{2} V _{2}}{T _{2}}

Ideal gas equation

P V = n R T

Avogadro constant

6.02 \times 1 0^{23} mol^{- 1}

Molar volume at STP

22.4 dm³/mol

Dilution

M_{1} V_{1} = M_{2} V_{2}

Elevation of boiling point

Δ T_{b} = K_{b} m

Depression of freezing point

Δ T_{f} = K_{f} m

pH and pOH

p H = - lo g [H^{+}]

;

p H + pO H = 14

at 25 °C

Equilibrium constant for

a A + b B ⇌ c C

K_{c} = \frac{[ C ] ^{c}}{[ A ] ^{a} [ B ] ^{b}}

Half-life of a first-order reaction

t_{1/2} = \frac{0.693}{k}

Order of a reaction

The sum of the powers of concentration in the rate law.

Faraday's constant

96500 C/mol of electrons.

Mass deposited in electrolysis

m = \frac{M}{n} \cdot \frac{I t}{96500}

Enthalpy of reaction from formation enthalpies

Δ H = \sum Δ H_{f} (products) - \sum Δ H_{f} (reactants)

Oxidation at the anode

Oxidation occurs at the anode and reduction at the cathode.

Nernst-type relation (qualitative)

A higher concentration of reactant ions raises the cell potential.

Le Chatelier's principle

A system at equilibrium shifts to oppose a change in conditions.

Effect of a catalyst on K

None; it speeds up forward and reverse reactions equally.

Moles from mass

n = m / M

Percentage by mass of an element

\frac{mass of element in formula}{formula mass} \times 100

Oxidation number of Mn in KMnO₄

Oxidation number of Cr in K₂Cr₂O₇

Oxidation number of S in H₂SO₄

Number of neutrons

Mass number − atomic number.

Combustion of methane

CH₄ + 2O₂ → CO₂ + 2H₂O, ΔH = −891 kJ/mol.

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