ΔG is related to Q by the equation ΔG=RTlnQK. If ΔG < 0, then K > Q, and the reaction must proceed to the right to reach equilibrium. If ΔG > 0, then K < Q, and the reaction must proceed to the left to reach equilibrium. If ΔG = 0, then K = Q, and the reaction is at equilibrium.
The correct answer is The rates of the forward and reverse reactions are equal. Chemical equilibrium, a condition in the course of a reversible chemical reaction in which no net change in the amounts of reactants and products occurs.
Shift to the right: a net reaction that converts reactants to product until equilibrium is reached. Shift to the left: a net reaction that converts product to reactant until equilibrium is reached.
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.
Kf=Kb is the correct answer.
Which of the following is true for a reaction at equilibrium? When a reaction is at equilibrium there is no further change in the concentrations of the reactants and products.
At equilibrium, the forward and backward rates of reaction are equal. So, the concentrations of the reactants and products are constant. Because - Concentration of reactants decreases and the concentration of products increases when the reaction proceeds.
6. What would happen to the equilibrium expressed by the reaction in Equation 11.8 if a reagent were added that lowered the Fe3+ ion concentration. a. Equilibrium would shift left.
This means if we add reactant, equilibrium goes right, away from the reactant. If we add product, equilibrium goes left, away from the product. If we remove product, equilibrium goes right, making product. If we remove reactant, equilibrium goes left, making reactant.
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?...EquationEquilibrium Constant N2(g) + O2(g) NO2(g)Kc = 4.1 x 10-92 more rows
A reaction can be 99% reactants, 1% products and be in equilibrium as long as those concentrations are not changing, and in that case the forward and reverse reaction rates are not equal.
The equilibrium constant for the reverse reaction is equal to the inverse of the equilibrium constant for the forward reaction.