Dalton's law

In chemistry and physics, Dalton's law (also called Dalton's law of partial pressures) states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.^[1] This empirical law was observed by John Dalton in 1801 and published in 1802.^[2] and is related to the ideal gas laws.

Formula

Mathematically, the pressure of a mixture of non-reactive gases can be defined as the summation:

p_{\text{total}}=\sum _{i=1}^{n}p_{i}

or

p_{\text{total}}=p_{1}+p_{2}+p_{3}+\cdots +p_{n}

where p₁, p₂, ..., p_n represent the partial pressures of each component.^[1]

p_{i}=p_{\text{total}}x_{i}

where x_i is the mole fraction of the ith component in the total mixture of n components.

Volume-based concentration

The relationship below provides a way to determine the volume-based concentration of any individual gaseous component

p_{i}=p_{\text{total}}c_{i}

where c_i is the concentration of the ith component.

Dalton's law is not strictly followed by real gases, with the deviation increasing with pressure. Under such conditions the volume occupied by the molecules becomes significant compared to the free space between them. In particular, the short average distances between molecules increases intermolecular forces between gas molecules enough to substantially change the pressure exerted by them, an effect not included in the ideal gas model.

References

^ ^a ^b Silberberg, Martin S. (2009). Chemistry: the molecular nature of matter and change (5th ed.). Boston: McGraw-Hill. p. 206. ISBN 9780073048598.
^ J. Dalton (1802), "Essay IV. On the expansion of elastic fluids by heat," Memoirs of the Literary and Philosophical Society of Manchester, vol. 5, pt. 2, pages 595–602; see page 600.

[Silberberg-1] Silberberg, Martin S. (2009). Chemistry: the molecular nature of matter and change (5th ed.). Boston: McGraw-Hill. p. 206. ISBN 9780073048598.

[2] J. Dalton (1802), "Essay IV. On the expansion of elastic fluids by heat," Memoirs of the Literary and Philosophical Society of Manchester, vol. 5, pt. 2, pages 595–602; see page 600.

[1]

[2]

v t e Distillation
Principles	Raoult's law Dalton's law Reflux Fenske equation McCabe–Thiele method Theoretical plate Partial pressure Vapor–liquid equilibrium
Industrial processes	Batch distillation Continuous distillation Fractionating column Spinning cone
Laboratory methods	Alembic Kugelrohr Rotary evaporator Spinning band distillation Still
Techniques	Azeotropic Catalytic Destructive Dry Extractive Fractional Reactive Salt-effect Steam-based Vacuum-based

Formula

Volume-based concentration

See also

References