NH4NO3 + H2O NH4NO3The reaction shown above is an endothermic reaction.Which of the following statements will be true, regardingequilibrium? Select all that apply.The kinetic energy of the product is higher than theactivation energy of the reactantsIf you add heat to this reaction, the equilibrium will shift tofavor the reverse reactionThe reaction is irreversibleIf you add heat to this reaction, the equilibrium will shift tofavor the forward reaction

Answered: Image /qna-images/answer/e3ef953b-3406-45a0-a953-dbd6cbeab57b.jpg

Answered: NH4NO3 + H2O NH4NO3 The reaction shown…

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter18: Chemical Equilibrium

Section: Chapter Questions

Problem 22E

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Similar questions

. In general terms. what does the equilibrium constant for a reaction represent? What is the algebraic form of the equilibrium constant for a typical reaction? What do square brackets indicate when we write an equilibrium constant?
Given the following descriptions of reversible reactions, write a balanced equation (smallest whole-number coefficients) and the equilibrium constant expression for each. (a) Nickel metal reacts with carbon monoxide to form nickel tetracarbonyl (Ni(CO)4) gas. (b) Aqueous nitrous acid in equilibrium with hydrogen and nitrite ions. (c) Chlorine gas and bromide ions in equilibrium with liquid bromine and chloride ions.
When molecules collide, a certain minimum energy called the _________ is needed for the reaction to occur.
When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate symbolically that the reaction is reversible?
Write equilibrium constant expressions for the following generalized reactions. a. 3X(g)+2Y(g)Z(g) b. 3X(g)+2Y(s)Z(g) c. 3X(s)+2Y(s)Z(g) d. 3X(g)+2Y(g)Z(s)
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.
Write an equilibrium expression for each of the following gaseous reactions: a.3O22O3 b.COCl2CO+Cl2 c.CS2+4H2CH4+2H2S d.2SO2+O22SO3 e.CO+H2OCO2+H2
. 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?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
Use Le Chteliers principle to predict the direction of equilibrium shift in the following equilibria when the indicated stress is applied: a. 2A+B+heatC; some A is removed. b. 2A+B+heatC+D; the system is cooled. c. N2O42NO2; some NO2 is removed.
Based on the diagrams, chemical reaction, and reaction conditions depicted in Problem 9-81, for which of the diagrams is the numerical value of the equilibrium constant the smallest?
. Suppose are action has the equilibrium constant K=1.3108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?

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