This chapter deals with chemical equilibrium, or how far chemical reactions proceed. Some reactions convert reactants to products with near 100% efficiency but others do not.
Chemical equilibrium is a dynamic process and occurs when the rates of two opposing processes (reactions) become the same. Unless conditions are somehow changed, the concentrations of both reactants and products remain constant after equilibrium is achieved.
Consider the decomposition reaction in which N2O4 (g) ' 2 NO2(g) What happens to the concentration of each, based upon the rate equations, as the reaction proceeds
Assuming reversible elementary processes, Rate (forward) = k (forward) x [N2O4] and rate (reverse) = k (reverse) x [NO2]2As [N2O4] decreases, rate forward decreases, and, as [NO2] increases, rate reverse increases, but more quickly.
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