Consider the reversible reaction: A+B=C+D What happens to the forward and reverse reaction rates when equilibrium is achieved? What happens to the reactant (A and B) and product (C and D) concentrations when equilibrium is achieved? LeChâtelier's Principle states that if a stress is applied to a reversible reaction at equilibrium, the reaction will undergo a shift in order to re-establish its equilibrium. Consider the following exothermic reversible reaction at equilibrium: 2 A=B+C In which direction (left or right) would the following stresses cause the system to shift? a. The concentration of A is decreased. b. The concentration of B is increased. c. The temperature of the system is lowered.

Consider the reversible reaction: A+B=C+D What happens to the forward and reverse reaction rates when equilibrium is achieved? What happens to the reactant (A and B) and product (C and D) concentrations when equilibrium is achieved? LeChâtelier's Principle states that if a stress is applied to a reversible reaction at equilibrium, the reaction will undergo a shift in order to re-establish its equilibrium. Consider the following exothermic reversible reaction at equilibrium: 2 A=B+C In which direction (left or right) would the following stresses cause the system to shift? a. The concentration of A is decreased. b. The concentration of B is increased. c. The temperature of the system is lowered.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Consider the exothermic reaction: C2H4(g) + I2(g) = C2H412(g) In trying to maximize the amount of C2H412 produced, which of the following will not work? Assume that the reaction mixture reaches equilibrium. O increasing the temperature O decreasing the volume of the reaction vessel O increasing the amount of C2H4 O adding more l2
Which of the following is true for a system whose equilibrium constant is much greater than one? The reaction mixture contains mostly products at equilibrium. The reaction mixture contains mostly reactants at equilibrium. O The rate of reaction is very fast. The moles of reactants and products are relatively similar at equilibrium. Both A and C.
Catalysts affect reaction rates, but do not change either the equilibrium or the spontaneity of a reaction. True or False.
I need these two
What role does a catalyst play in a reversible chemical reaction? How does a catalyst affect the value of the equilibrium constant for a reaction?
Select all of the correct statements about equilibrium from the choices below.At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the forward rate drops. At equilibrium all reactions stop. Reactants are transformed into products even at equilibrium. As a reaction proceeds forward toward equilibrium the reverse rate constant rises.As a reaction proceeds forward toward equilibrium the forward rate constant drops.
What is the difference between a reversible and an irreversible reaction?
which statement is true?
Consider the following reversible reaction at equilibrium: CO(g) + Cl2(g) COCI,(g). Use Le Chatelier's principle to predict the effect of adding some Cl2(g) to the equilibrium system? the concentration of CO(g) increases the concentration of COC12(g) decreases the equilibrium system shifts to the right to restore equilibrium the equilibrium system shifts to the left to restore equilibrium no effect
The oxidation of ammonia is a reversible exothermic reaction at equilibrium that proceeds as follows: 4 NH3 (g) + 5 O2 (g) ⇋ 4 NO (g) + 6 H2O (g) If the temperature is decrease, what happens to the concentration of H2O?
Can you show me how to answer this type of question I found on a online practice organic chemistry review.
For any reversible reaction containing a double arrow such as: Reactants ⟷⟷ Products the statement "equilibrium shifts to the right" means: Group of answer choices; - The reaction can only go in the forward direction. - The reaction can only go in the reverse direction. - A stress will cause a portion of reactants to disappear and some additional products to appear. - A stress will cause a portion of products to disappear and some additional reactants to appear