Equillibrium Definition

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  • Equilibrium definitions
    • A chemical reaction is in equilibrium when the concentrations of the reactants and the products are contant and the forwars and reverse reactions occur at equal rates.
    • Equilibrium position - a condition in which all acting influences are cancelled by others, resulting in a stable, balanced or unchanging system.
    • Reversible reaction - A reaction in the backwards directions, reaction in which original reactants emerge again from the products. It goes from riight to left.
    • Products - The substanced that result from the recombination of atoms.
    • Completion - The limiting reactants are used up.
    • Forward reactions - a reaction in which products are produced from reactants and it goes from left to right in a reversible reaction.
    • A reversible reaction - A reversible reaction is a reaction where the reactants form products, which react together to give the reactants back.
    • Rate of reaction - the speed at which a chemical reaction proceeds.
    • Dynamic Equilibrium - exists once a reversible reation ceases to change its ratio of reacants / procucts, but substances move between the chemicals at an equal rate, meaning there is not net change.
    • Reactants - Substances (elements and/or compunds) which are changed into other substanced (comppunds and/or elements) called poducts.
    • A closed system - a physical system that does not allow certain types of transfers (such as transfer of mass and energy transfers) in or out of the system.
    • Concentration - Refers to the amount of a substance per unit mass.

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