Energy is absorbed to break bonds. Bond-breaking is an endothermic process. Energy is released when new bonds form. Bond-making is an exothermic process. The equilibrium constant shows how far the reaction will progress at a specific temperature by determining the ratio of products to reactions using equilibrium concentrations. The equilibrium expression for the following equation. If the products dominate in a reaction, the value for K is greater than 1.
The larger the K value, the more the reaction will tend toward the right and thus to completion. Suppose that the following reaction is at equilibrium and that the concentration of N 2 is 2 M, the concentration of H 2 is 4 M, and the concentration of NH 3 is 3 M.
What is the value of K c? For the previous equation, does the equilibrium favor the products or the reactants? As such, the change in enthalpy for an endothermic reaction is always positive. In order to melt the ice cube, heat is required, so the process is endothermic. Whether a reaction is endothermic or exothermic depends on the direction that it is going; some reactions are reversible, and when you revert the products back to reactants, the change in enthalpy is opposite.
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Exothermic and Endothermic Processes. Learning Objective Distinguish between endothermic and exothermic reactions.
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