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13 Νοε 2022 · A chemical reaction is in equilibrium when there is no tendency for the quantities of reactants and products to change. The direction in which a chemical reaction is written (and thus which components are considered reactants and which are products) is arbitrary. Consider the following two reactions:
29 Σεπ 2024 · An example of a reaction reaching equilibrium is the reaction between H 2 and N 2 in the Haber process: At the start of the reaction, only nitrogen and hydrogen are present. This means that the rate of the forward reaction is at its highest, since the concentrations of hydrogen and nitrogen are at their highest.
12 Σεπ 2022 · A mixture of reactants and products is found at equilibrium. For example, when we place a sample of dinitrogen tetroxide (\(N_2O_4\), a colorless gas) in a glass tube, it forms nitrogen dioxide (\(\ce{NO2}\), a brown gas) by the reaction \[\ce{ N2O4(g) \rightleftharpoons 2NO2(g)} \label{13.2.1} \]
At equilibrium, the forward and reverse reactions proceed at equal rates. Consider, for example, a simple system that contains only one reactant and one product, the reversible dissociation of dinitrogen tetroxide (N2O4 N 2 O 4) to nitrogen dioxide (NO2 NO 2).
In a chemical reaction, chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time, so that there is no observable change in the properties of the system. [1]
Describe examples of systems involving two (or more) simultaneous chemical equilibria. Calculate reactant and product concentrations for multiple equilibrium systems. Compare dissolution and weak electrolyte formation. There are times when one equilibrium reaction does not adequately describe the system being studied.
In this lecture, we discuss the nature of chemical equilibrium and of the chemical equilibrium constant. We start to consider how external factors can “push” the equilibrium in one direction or the other.
