two substances are combined and react. After 10 minutes the chemical reaction has reached equilibrium which values would be equal to zero for the solution
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In a chemical reaction that has reached equilibrium, it means that the forward and reverse reactions are occurring at the same rate and there is no net change in the concentration of the reactants and products over time. At equilibrium, various properties, such as concentration, are constant and do not change further.
To determine which values would be equal to zero for the solution at equilibrium, you need to understand the concept of equilibrium constants. The equilibrium constant, denoted as K, is a numerical value that relates the concentrations of the reactants and products at equilibrium. It is expressed as the ratio of the products' concentrations to the reactants' concentrations, where each component is raised to the power of its stoichiometric coefficient in the balanced chemical equation.
For example, consider the generic reaction:
aA + bB ⇌ cC + dD
The equilibrium constant expression for this reaction can be written as:
K = ([C]^c * [D]^d) / ([A]^a * [B]^b)
In this equation, [A], [B], [C], and [D] denote the concentrations of the corresponding substances at equilibrium. The stoichiometric coefficients a, b, c, and d represent the number of moles of each component involved in the reaction.
For a given reaction, if the equilibrium constant (K) is equal to zero, it implies that the concentrations of the products ([C] and [D]) are zero, while the concentrations of the reactants ([A] and [B]) may or may not be zero. Therefore, at equilibrium, the values of [C] and [D] would be zero for the solution.
It is important to note that not all chemical reactions will have equilibrium constants that are equal to zero. The specific equilibrium constant value depends on the reaction and its stoichiometry.