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The reaction quotient is the ratio of products to reactants not at equilibrium. If the system is at equilibrium then Q becomes Keq the equilibrium constant.

Q = products/reactants

If Q < Keq then there are more reactants then products so the system must shift toward the products to achieve equilibrium.

If Q > Keq then there are more products than reactants and the system must shift toward the reactants to reach equilibrium.

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14y ago

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The reaction quotient indicates what?

The reaction quotient indicates the relative amounts of products and reactants present in a system at a given time compared to what would be present at equilibrium. It helps determine the direction a reaction will shift to reach equilibrium.


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How can one determine the reaction quotient in a chemical reaction?

To determine the reaction quotient in a chemical reaction, you need to calculate the concentrations of the reactants and products at a specific point in time. The reaction quotient is calculated using the same formula as the equilibrium constant, but with the concentrations of the reactants and products at that specific point in time. This helps determine whether the reaction is at equilibrium or not.


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To calculate the reaction quotient in a chemical reaction, you need to multiply the concentrations of the products raised to their respective coefficients, and then divide by the concentrations of the reactants raised to their respective coefficients. This helps determine if a reaction is at equilibrium or not.


The reaction quotient Q indicates?

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What is the reaction quotient q?

The reaction quotient, denoted as ( Q ), is a measure of the relative concentrations of reactants and products in a chemical reaction at any given point in time, not necessarily at equilibrium. It is calculated using the same expression as the equilibrium constant ( K ), with the concentrations of products and reactants raised to the power of their stoichiometric coefficients. By comparing ( Q ) to ( K ), one can determine the direction in which the reaction will proceed to reach equilibrium. If ( Q &lt; K ), the reaction will shift to the right (toward products); if ( Q &gt; K ), it will shift to the left (toward reactants).


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How can a chemical reaction shift toward the desired direction?

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What is true about a solution if the reaction quotient is less than the solubility product constant?

the reaction is at dynamic equilibrium.


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Direction Reaction Creation was created in 1977-03.


What is the relationship between the standard free energy change (G), the equilibrium constant (Keq), and the reaction quotient in the context of the G G RTln(Q) equation?

The standard free energy change (G), the equilibrium constant (Keq), and the reaction quotient (Q) are related through the equation G G RTln(Q). This equation shows how the actual free energy change (G) of a reaction relates to the standard free energy change (G) at equilibrium, the gas constant (R), the temperature (T), and the natural logarithm of the reaction quotient (Q). The equilibrium constant (Keq) is related to Q and G through this equation, providing insight into the spontaneity and direction of a chemical reaction.