Will the rate of the forward reaction exceed the rate of the reverse reaction before equilibrium is reestablished?

If the concentrations of the reactants are too large for the reaction to be at equilibrium, the rate of the forward reaction will be faster than the reverse reaction, and some of the reactants will be converted into products until equilibrium is achieved.

Why the rate of forward reaction is greater than reverse reaction?

If the rate of the forward reaction is greater than the rate of the reverse reaction, that means there’s a net conversion of reactants to products. So therefore over time, the amount of reactants would decrease and the amount of products would increase.

How do the rates of the forward and reverse reactions compare at equilibrium?

At equilibrium: The rate of the forward reaction is equal to the rate of the reverse reaction. No further changes occur in the concentrations of reactants and products, even though the two reactions continue at equal but opposite rates.

What happens to the rate of the forward reaction compared with the backward reaction?

the rates of the forward and backward reactions are the same. the concentrations of the reactants and products remain constant (they do not change)

Does the rate of the forward reaction increase or decrease until equilibrium is reached?

The forward reaction rate will increase sharply, and then gradually decrease until equilibrium is re-established. At the same time the reverse reaction rate will gradually increase. An increase in product concentration will favour the reverse reaction.

What happens to the rate of the forward reaction as the reactants are consumed?

As reactants are consumed and products are formed, the rate of the forward reaction decreases and the rate of the reverse reaction increases. Eventually, the two rates must become equal.

Why does the rate of forward reaction decrease with time?

The rate of a reaction decreases as time progresses. As a reaction progresses the reactants are being turn junto the products, so the number of reactant particles left is decreasing.

When the rate of the forward reaction equals the rate of the backward reaction system is said to be in 2 points?

Chemical equilibrium
Chemical equilibrium is a state in which the rate of the forward reaction equals the rate of the backward reaction. In other words, there is no net change in concentrations of reactants and products. This kind of equilibrium is also called dynamic equilibrium.

Why does the forward reaction decrease as equilibrium is approached?

Why does the forward reaction rate decrease as equilibrium is approached? As the reaction goes to the right, the reaction concentration decreases and therefore, there are less reactant collisions causing the forward rate to decrease.

How do the rates of forward and backward reactions become same?

For reversible reactions, initially the products are formed at a faster rate but then with time even the backward reaction starts . A stage comes where the concentration of both , reactants and products become same , that’s when we say that equilibrium is achieved and at equilibrium, rates of forward and backward reactions becomes same .

What happens to the rate of reverse reaction as Hi increases?

As HI builds up, the rate of the reverse reaction increases, while the rate of the forward reaction decreases (not as much H2 and I2 to react as often). Eventually the rates become equal, which means the reaction has reached equilibrium.

What happens to reactants and products at equilibrium?

At equilibrium, both reactants and products are present. oSome reaction mixtures contain mostly reactants and form only a few products at equilibrium. oSome reaction mixtures contain mostly products and remain mostly reactants at equilibrium. Equilibrium:The rate of the forward reaction and the rate of the reverse reaction are equal.

What is the rate constant of a reversible reaction?

For a reversible reaction the rate constant for forward and backward reaction are 2.38 * 10 ^ -4 and 8.15 * 10 ^-5 respectively. thermodynamically favorable compared with the reverse reaction and thus the relationship k1>=k2 maintains between the rate constants.