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4.3 Concentration and Pressure

  • Page ID
    32227
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    Increasing the concentration of any one or more of the reactants will usually (but not always) increase the rate of a reaction if the reactants are all in the same phase (solid, liquid, gas, or aqueous).

    Why? Concentration is a measure of how many particles are in a given volume. By packing more particles in the same space, collisions will occur more often, thus increasing the rate of the reaction.

    Remember our thought experiment with blindfolded students in a room? You would demonstrate how concentration increases reaction rate by packing more blindfolded students into that room.

    The concentration of gases is typically increased by decreasing the volume (making the container smaller). This forces the particles closer together, thus increasing their concentration.

    Changing the concentration, or increasing the pressure, does not affect the amount of energy particles collide with. It simply increases the rate by increasing the frequency of collisions.

    Changes in concentration also explain why the rate of a reaction slows down as a reaction proceeds. As the reactant particles collide with one another to form products, there are fewer and fewer reactant particles as the reaction continues. This lowers their concentration (fewer particles in a given volume), thus the rate declines.


    Note:

    Concentration (as was mentioned in section 1-3) is commonly measured as molarity, with the symbol M
    (the units for molarity are mol / L or mol·L
    -1).

    A 6 M solution (containing 6 moles of a substance dissolved in 1 litre of solution) is more concentrated than a 1 M solution
    (1 mole of the substance dissolved in 1 litre of solution).


    4.3 Concentration and Pressure is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts.

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