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R is the gas constant and T is the absolute temperature. Note that pK a = −log(K a) and 2.303 ≈ ln(10). At 25 °C, ΔG ⊖ in kJ·mol −1 ≈ 5.708 pK a (1 kJ·mol −1 = 1000 joules per mole). Free energy is made up of an enthalpy term and an entropy term. [11] =
1.358 0.02789 Nitrogen: 1.370 0.0387 Nitrogen dioxide: 5.354 0.04424 Nitrogen trifluoride [2] 3.58 0.0545 Nitrous oxide: 3.832 0.04415 Octane [2] 37.88 0.2374 1-Octanol [2] 44.71 0.2442 Oxygen: 1.382 0.03186 Ozone [2] 3.570 0.0487 Pentane: 19.26 0.146 1-Pentanol [2] 25.88 0.1568 Phenol [2] 22.93 0.1177 Phosphine: 4.692 0.05156 Propane: 8.779 0. ...
The higher the proton affinity, the stronger the base and the weaker the conjugate acid in the gas phase.The (reportedly) strongest known base is the ortho-diethynylbenzene dianion (E pa = 1843 kJ/mol), [3] followed by the methanide anion (E pa = 1743 kJ/mol) and the hydride ion (E pa = 1675 kJ/mol), [4] making methane the weakest proton acid [5] in the gas phase, followed by dihydrogen.
The gas constant occurs in the ideal gas law: = = where P is the absolute pressure, V is the volume of gas, n is the amount of substance, m is the mass, and T is the thermodynamic temperature. R specific is the mass-specific gas constant. The gas constant is expressed in the same unit as molar heat.
This list is sorted by boiling point of gases in ascending order, but can be sorted on different values. "sub" and "triple" refer to the sublimation point and the triple point, which are given in the case of a substance that sublimes at 1 atm; "dec" refers to decomposition. "~" means approximately.
The solvent (e.g. water) is omitted from this expression when its concentration is effectively unchanged by the process of acid dissociation. The strength of a weak acid can be quantified in terms of a dissociation constant , K a {\displaystyle K_{a}} , defined as follows, where [ X ] {\displaystyle {\ce {[X]}}} signifies the concentration of a ...
Δ r G, Gibbs free energy change per mole of reaction, Δ r G°, Gibbs free energy change per mole of reaction for unmixed reactants and products at standard conditions (i.e. 298 K, 100 kPa, 1 M of each reactant and product), R, gas constant, T, absolute temperature, ln, natural logarithm, Q r, reaction quotient (unitless),
The concentration of the species LH is equal to the sum of the concentrations of the two micro-species with the same chemical formula, labelled L 1 H and L 2 H. The constant K 2 is for a reaction with these two micro-species as products, so that [LH] = [L 1 H] + [L 2 H] appears in the numerator, and it follows that this macro-constant is equal ...