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  2. Ideal gas law - Wikipedia

    en.wikipedia.org/wiki/Ideal_gas_law

    The state of an amount of gas is determined by its pressure, volume, and temperature. The modern form of the equation relates these simply in two main forms. The temperature used in the equation of state is an absolute temperature: the appropriate SI unit is the kelvin. [4]

  3. Enthalpy - Wikipedia

    en.wikipedia.org/wiki/Enthalpy

    Enthalpy (/ ˈ ɛ n θ əl p i / ⓘ) is the sum of a thermodynamic system's internal energy and the product of its pressure and volume. [1] It is a state function in thermodynamics used in many measurements in chemical, biological, and physical systems at a constant external pressure, which is conveniently provided by the large ambient atmosphere.

  4. Relations between heat capacities - Wikipedia

    en.wikipedia.org/wiki/Relations_between_heat...

    P = pressure V = volume n = number of moles R = universal gas constant T = temperature. The ideal gas equation of state can be arranged to give: = / or = / The following partial derivatives are obtained from the above equation of state:

  5. Fundamental thermodynamic relation - Wikipedia

    en.wikipedia.org/wiki/Fundamental_thermodynamic...

    Thus, they are essentially equations of state, and using the fundamental equations, experimental data can be used to determine sought-after quantities like G (Gibbs free energy) or H . [1] The relation is generally expressed as a microscopic change in internal energy in terms of microscopic changes in entropy , and volume for a closed system in ...

  6. Van 't Hoff equation - Wikipedia

    en.wikipedia.org/wiki/Van_'t_Hoff_equation

    The Van 't Hoff equation relates the change in the equilibrium constant, K eq, of a chemical reaction to the change in temperature, T, given the standard enthalpy change, Δ r H ⊖, for the process. The subscript r {\displaystyle r} means "reaction" and the superscript ⊖ {\displaystyle \ominus } means "standard".

  7. Thermodynamic equations - Wikipedia

    en.wikipedia.org/wiki/Thermodynamic_equations

    Entropy cannot be measured directly. The change in entropy with respect to pressure at a constant temperature is the same as the negative change in specific volume with respect to temperature at a constant pressure, for a simple compressible system. Maxwell relations in thermodynamics are often used to derive thermodynamic relations. [2]

  8. Hess's law - Wikipedia

    en.wikipedia.org/wiki/Hess's_law

    The law states that the total enthalpy change during the complete course of a chemical reaction is independent of the sequence of steps taken. [2] [3] Hess's law is now understood as an expression of the fact that the enthalpy of a chemical process is independent of the path taken from the initial to the final state (i.e. enthalpy is a state ...

  9. Isobaric process - Wikipedia

    en.wikipedia.org/wiki/Isobaric_process

    For a thermally perfect diatomic gas, the molar specific heat capacity at constant pressure (c p) is 7 / 2 R or 29.1006 J mol −1 deg −1. The molar heat capacity at constant volume (c v) is 5 / 2 R or 20.7862 J mol −1 deg −1. The ratio of the two heat capacities is 1.4. [4] The heat Q required to bring the gas from 300 to 600 K is