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A chemical equilibrium is established when two exactly opposite reactions occur in the same container at the same time and with the same rates of reaction. At equilibrium the concentrations of the chemical species become constant, but not necessarily equal. For the reaction aA + bB Kc =
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In this expression, k is the rate constant a constant for each chemical reaction at a given temperature. The exponents m and n, called the orders of reaction, indicate what effect a change in concentration of that reactant species will have on the reaction rate. Say, for example, m = 1 and n = 2. That means that if the concentration of reactant A is dou1 bled, then the rate will also double ([2] = 2), and if the concentration of reactant B is dou2 bled, then the rate will increase fourfold ([2] = 4). We say that it is first order with respect to A and second order with respect to B. If the concentration of a reactant is doubled and that has no effect on the rate of reaction, then the reaction is zero order with respect to that 0 reactant ([2] = 1). Many times the overall order of reaction is calculated; it is simply the sum of the individual coefficients, third order in this example. The rate equation would then be shown as:
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