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  2. Dynamic equilibrium (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Dynamic_equilibrium...

    In chemistry, a dynamic equilibrium exists once a reversible reaction occurs. Substances initially transition between the reactants and products at different rates until the forward and backward reaction rates eventually equalize, meaning there is no net change.

  3. Reversible reaction - Wikipedia

    en.wikipedia.org/wiki/Reversible_reaction

    Weak acids and bases undergo reversible reactions. For example, carbonic acid: H 2 CO 3 (l) + H 2 O (l) ⇌ HCO 3 − (aq) + H 3 O + (aq). The concentrations of reactants and products in an equilibrium mixture are determined by the analytical concentrations of the reagents (A and B or C and D) and the equilibrium constant, K.

  4. Chemical equilibrium - Wikipedia

    en.wikipedia.org/wiki/Chemical_equilibrium

    If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to partially reverse the change. For example, adding more S (to the chemical reaction above) from the outside will cause an excess of products, and the system will try to counteract this by increasing the reverse reaction and pushing the ...

  5. Randles–Sevcik equation - Wikipedia

    en.wikipedia.org/wiki/Randles–Sevcik_equation

    In electrochemistry, the Randles–Ševčík equation describes the effect of scan rate on the peak current (i p) for a cyclic voltammetry experiment. For simple redox events where the reaction is electrochemically reversible, and the products and reactants are both soluble, such as the ferrocene/ferrocenium couple, i p depends not only on the concentration and diffusional properties of the ...

  6. Transition state theory - Wikipedia

    en.wikipedia.org/wiki/Transition_state_theory

    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.

  7. Energy profile (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Energy_profile_(chemistry)

    A reaction is in equilibrium when the rate of forward reaction is equal to the rate of reverse reaction. Such a reaction is said to be reversible. If the starting material and product(s) are in equilibrium then their relative abundance is decided by the difference in free energy between them.

  8. Curtin–Hammett principle - Wikipedia

    en.wikipedia.org/wiki/Curtin–Hammett_principle

    The Curtin–Hammett principle is a principle in chemical kinetics proposed by David Yarrow Curtin and Louis Plack Hammett.It states that, for a reaction that has a pair of reactive intermediates or reactants that interconvert rapidly (as is usually the case for conformational isomers), each going irreversibly to a different product, the product ratio will depend both on the difference in ...

  9. Microscopic reversibility - Wikipedia

    en.wikipedia.org/wiki/Microscopic_reversibility

    In chemistry, J. H. van't Hoff (1884) [4] came up with the idea that equilibrium has dynamical nature and is a result of the balance between the forward and backward reaction rates. He did not study reaction mechanisms with many elementary reactions and could not formulate the principle of detailed balance for complex reactions.