Question

At equilibrium the reactant and product concentrations are constant because a change in one direction is balanced by a change in the other as the forward and reverse rates become equal:At equilibrium: rate_twd=rate_rev When a chemical system is at equilibrium,a. he concentrations of the reactants and products have reached constant values.b. the concentrations of the reactants are equal to the concentrations of the products.c. the forward and reverse reactions have stopped.d. the reaction quotient, Q, has reached a maximum.e. None of the choices.

Answer 1

At equilibrium, reactant and product concentrations remain constant, indicating a dynamic balance between the forward and reverse reactions. The concentrations of reactants and products are not equal, but their rates of formation are. The reaction quotient Q represents the ratio of product and reactant concentrations at any given time and equals the constant K at equilibrium.

Step-by-step explanation:

At equilibrium, the rate of the forward reaction becomes equal to the rate of the reverse reaction, known as the point of dynamic equilibrium. In this state, the concentrations of the reactants and products are constant. This does not mean the concentrations of the reactants are equal to the concentrations of the products; instead, they are not changing. Although the system may appear inactive, the forward and reverse reactions continue to occur at an equal rate. As a result, the reaction quotient, Q, represents the ratio of the concentrations of the products to the reactants for a reaction at a given time and remains constant at equilibrium. However, Q does not reach a maximum but stabilizes to a constant value known as the equilibrium constant, K.

Answer 2

Answer: a. The concentrations of the reactants and products have reached constant values

Step-by-step explanation:

The reactions which do not go on completion and in which the reactant forms product and the products goes back to the reactants simultaneously are known as equilibrium reactions. For a chemical equilibrium reaction, equilibrium state is achieved when the rate of forward reaction becomes equal to rate of the backward reaction.

Equilibrium state is the state when reactants and products are present but the concentrations does not change with time and are constant.

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
`K_(eq)`

K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For a equilibrium reaction,

`A\rightleftharpoons B`

`K_(eq)=([B])/([A])`

Thus the correct answer is the concentrations of the reactants and products have reached constant values.