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In biochemistry, steady state refers to the maintenance of constant internal concentrations of molecules and ions in the cells and organs of living systems. [1] Living organisms remain at a dynamic steady state where their internal composition at both cellular and gross levels are relatively constant, but different from equilibrium concentrations. [1]
Donnan equilibrium across a cell membrane (schematic). The Gibbs–Donnan effect (also known as the Donnan's effect, Donnan law, Donnan equilibrium, or Gibbs–Donnan equilibrium) is a name for the behaviour of charged particles near a semi-permeable membrane that sometimes fail to distribute evenly across the two sides of the membrane. [1]
In biology, homeostasis (British also homoeostasis; / h ɒ m i oʊ ˈ s t eɪ s ɪ s,-m i ə-/ hoh-mee-oh-STAY-sis) is the state of steady internal physical and chemical conditions maintained by living systems. [1]
The balance of nature, also known as ecological balance, is a theory that proposes that ecological systems are usually in a stable equilibrium or homeostasis, which is to say that a small change (the size of a particular population, for example) will be corrected by some negative feedback that will bring the parameter back to its original "point of balance" with the rest of the system.
In 1884, Jacobus van 't Hoff proposed the Van 't Hoff equation describing the temperature dependence of the equilibrium constant for a reversible reaction: = where ΔU is the change in internal energy, K is the equilibrium constant of the reaction, R is the universal gas constant, and T is thermodynamic temperature.
In this ecological context, hysteresis refers to the existence of different stable states under the same variables or parameters. Hysteresis can be explained by "path-dependency", in which the equilibrium point for the trajectory of "A → B" is different from for "B → A". In other words, it matters which way the ball is moving across the ...
At equilibrium, the rate of transfer of CO 2 from the gas to the liquid phase is equal to the rate from liquid to gas. In this case, the equilibrium concentration of CO 2 in the liquid is given by Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. [1]
E eq,K + is the equilibrium potential for potassium, measured in volts; R is the universal gas constant, equal to 8.314 joules·K −1 ·mol −1; T is the absolute temperature, measured in kelvins (= K = degrees Celsius + 273.15) z is the number of elementary charges of the ion in question involved in the reaction