Study-note-5-53 - 14.1 Define chemical equilibrium Concentrations of reactants and products remain constant A chemical equilibrium is “dynamic”

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Unformatted text preview: 14.1 Define chemical equilibrium. Concentrations of reactants and products remain constant. A chemical equilibrium is “dynamic”. What does this indicate? Reactants and products continue to form. An equilibrium exists because forward and reverse reactions occur at equal rates. How are equilibrium reactions written differently than other chemical reactions? They are written with instead of → . For example: Chemical reaction: A + B → C Equilibrium reaction: A + B C Explain how an equilibrium forms from pure reactants. As reactants combine to form products, 1) the concentration of reactants decreases, slowing the rate of the forward reaction, 2) the concentration of products increases, speeding the rate of the reverse reaction. Eventually both rates will be equal. Graph the formation of a dynamic equilibrium from pure reactants. Label the axes. Indicate with an arrow where equilibrium begins....
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This note was uploaded on 04/12/2011 for the course CHEM 1010 taught by Professor Marshall during the Spring '11 term at North Texas.

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