Abstract
This chapter describes equilibrium constant expressions and explains how to formulate them. It discusses the influence on equilibrium of temperature, pressure, and concentration. The chapter presents a general method for solving equilibrium constant problems. Equilibrium reactions are important in most areas of chemistry, and the chapter describes calculations based on them. Any reversible chemical reaction can achieve equilibrium. An initial mixture of reactants of any concentrations reaches equilibrium, such that the concentrations of reactants and products are related by the law of chemical equilibrium. The chapter explains LeChatelier's principle and the comparison of variations in equilibrium constants, rate constants, and rates. Mixtures of all kinds of substances, such as biochemical fluids, inorganic salts, organic compounds, and polymers, can be separated by the various types of chromatography. The purpose of the separation might simply be to find out how many substances are in a mixture. The equilibrium constant for the distribution of a solute between the two immiscible solvents is called “distribution coefficient.” The chapter illustrates Haber process for the manufacture of ammonia.
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