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Dynamic equilibriums occur for reversible reactions. They happen when sufficient product is formed that the rate of the reverse reaction becomes as great as the rate of the forward reaction. The result is zero net change in product and reactant concentrations. In a dynamic equilibrium: 1. The rate of forward reaction = Rate of backward reaction 2. The concentration of products and reactants remain constant 3. The reaction exists within a closed system (No reactant enters, no product leaves) This is routinely asked in A level chemistry examinations. That’s all!
Some reactions are able to go in two directions; forward and reverse. They are known as reversible reactions. When the rate of the forward reaction is equal to the rate of the reverse reaction, the reaction is said to have reached a dynamic equilibrium. In a dynamic equilibrium the ratios of reactants/products no longer change as reactants are being converted to products and products are being turned into reactants at the same time. As a result, there is no net change.
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