Select all the TRUE statements about chemical equilibrium. At equilibrium the rates of the forward and reverse reactions are equal. At equilibrium the concentrations of reactants and products remain constant. At equilibrium the reactants are still being converted to products (and vice versa). At equilibrium the concentrations of reactants and products are equal.

Select all the TRUE statements about chemical equilibrium. At equilibrium the rates of the forward and reverse reactions are equal. At equilibrium the concentrations of reactants and products remain constant. At equilibrium the reactants are still being converted to products (and vice versa). At equilibrium the concentrations of reactants and products are equal.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 10CR: . Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why...

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. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
Consider the following equilibrium system. N2(g)+O2(g)2NO(g) a. Write the chemical equation for the forward reaction. b. Write the chemical equation for the reverse reaction.
Tell what will happen to each equilibrium concentration in the following when the indicated stress is applied and a new equilibrium position is established. a. LiOH(s)+CO2(g)LiHCO3(s)+heat; CO2 is removed. b. 2NaHCO3(s)+heatNa2O(s)+2CO2(g)+H2O(g); The system is cooled. c. CaCO3(s)+heatCaO(s)+CO2(g); The system is cooled.
For the generalized chemical reaction A(g)+B(g)C(g)+D(g) determine whether the concentration of A in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a. concentration of B is increased b. concentration of C is decreased c. concentration of D is increased d. concentration of D is decreased
Write a balanced chemical equation for a totally gaseous equilibrium system that would lead to the following equilibrium constant expression. Keq=[N2]2[H2O]6[NH3]4[O2]3
Indicate whether or not each of the following changes would affect the value of a systems equilibrium constant. a. Addition of a product to the equilibrium mixture b. Increase in the systems total pressure c. Increase in the systems temperature d. Addition of both a reactant and a product to the equilibrium mixture
For the equilibrium reaction in Question 4, write the expression for the equilibrium constant. (a) How would this equilibrium constant change if the total pressure on the system were doubled? (b) How would the equilibrium constant change if the temperature were increased?