Select all of the true statements regarding chemical equilibrium. Select one or more: The rates of the forward and reverse reactions are equal. The concentrations of reactants and products are equal. Reactants are being converted to products and vice versa. The concentrations of reactants and products remain constant. Next
Choice B, C, and D.
Choice A is not true in general. Here's a way to think about that. Consider a very special equilibrium where the concentration of reactants and products are indeed equal. When one of the external factors (such as temperature) changes, the equilibrium will shift towards either side of the reaction. More products will be converted to reactants, or vice versa. Either way, in the new equilibrium, the concentration of the reactants and products will not be equal any more.
Choice B should be considered with choice C and D in mind.
Choice C is indeed correct. The reaction rate would not be zero unless all the reactants were used up or taken out of the system. That's not what happens in an equilibrium. Instead, when reaction rate is plotted against time, the graph for reactions in both directions will eventually flat out at a non-zero value.
Choice D explains why even though choice C is correct, the concentration of a system at equilibrium stays the same. At the equilibrium, reactions in both directions are still happening. However, during the time it takes for the forward reaction use up some reactant particles, the reverse reaction would have produced these particles again. On a large scale, there would be no observable change to the concentration of each species in the equilibrium. Therefore, choice B is also correct.
The correct statements are:
The concentrations of reactants and products remain constant.Reactants are being converted to products and vice versa. The rates of the forward and reverse reactions are equal.
Equilibrium defined as state of the reversible reaction where extend of reaction moving froward is equal to the extend of reaction moving backwards.
The rate reaction going forward is equal to the rate of the reaction going backward.At equilibrium state the concentration of reactants and products remain constant.Ratio of concentration of products to reactants raised to the power equal to their stoichiometric coefficient is always constant and termed as equilibrium constant.
The concentrations of reactants and products remain constant. The rates of the forward and reverse reactions are equal.
Chemical equilibrium is the state of a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction. While a reaction is in equilibrium the concentration of the reactants and products are constant. ... There are many examples of chemical equilibrium all around you.
The equilibrium constant of a chemical reaction is the value of the reaction quotient when the reaction has reached equilibrium. An equilibrium constant value is independent of the concentrations of the reactant and product species in a mixture but depends on temperature and on ionic strength.
Temperature increase favours the endothermic reaction.
-first ( A ) the concentrations of reactants and products are equal is false, As the concentrations of reactants and products may be different from each other.
- But (B) the concentrations of reactants and product remains constant is true, as the equilibrium remains when there is no change in the concentration of the reactants and products.
-(c) reactants are being converted to products (and vise verse) is true also, as there are reactions still happened at a constant rate so it looks like nothing is happening.