Why should rates of forward and reverse reaction become equal in equilibrium?
(c) At equilibrium, the forward and reverse reaction rates are equal. As the reaction begins (t = 0), the concentration of the N2O4 reactant is finite and that of the NO2 product is zero, so the forward reaction proceeds at a finite rate while the reverse reaction rate is zero.
How are the equilibrium constants for the forward and reverse reactions related?
The equilibrium constant is equal to the rate constant for the forward reaction divided by the rate constant for the reverse reaction.
Are the rates of the forward and reverse reactions the same?
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.
Is the forward or reverse reaction faster at equilibrium?
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.
Do the forward and reverse reactions stop at equilibrium?
In a chemical equilibrium, the forward and reverse reactions do not stop, rather they continue to occur at the same rate, leading to constant concentrations of the reactants and the products. We can detect a state of equilibrium because the concentrations of reactants and products do not appear to change.
Is a system at equilibrium if the rate constant of the forward and reverse reactions are equal?
A system is at equilibrium when the rates of the forward and reverse reactions are equal. If additional reactant is added the rate of the forward reaction increases. As the rate of the reverse reaction is initially unchanged, the equilibrium appears to shift toward the product, or right, side of the equation.
What is the equilibrium constant for a reverse reaction?
The equilibrium expression written for a reaction written in the reverse direction is the reciprocal of the one for the forward reaction. K’ is the constant for the reverse reaction and K is that of the forward reaction. N2O4(g) at 100o C?…
| Equation | Equilibrium Constant |
|---|---|
| N2(g) + O2(g) NO2(g) | Kc = 4.1 x 10-9 |
What is a forward reaction and reverse reaction in equilibrium?
Key points. A reversible reaction can proceed in both the forward and backward directions. Equilibrium is when the rate of the forward reaction equals the rate of the reverse reaction. All reactant and product concentrations are constant at equilibrium.
Is equilibrium is achieved when the forward reaction rate equals the reverse reaction rate?
Chemical equilibrium occurs when the rate of a forward chemical reaction is equal to the rate of reverse reaction while the concentrations of products and reactants remain unchanged.
When any reversible reaction is at equilibrium?
Reversible reactions that happen in a closed system eventually reach equilibrium. At equilibrium, the concentrations of reactants and products do not change. But the forward and reverse reactions have not stopped – they are still going on, and at the same rate as each other.
What do the rates of the forward and backward reactions in a reversible reaction depend on?
A reversible reaction is one in which reactants form products and at the same time products are forming reactants. When some products are formed, some of it will react to reform the reactants. And the rate of the forward reaction begins to decrease. As more product forms, so the rate of the backward reaction increases.