What is meant when a reaction is described as “having reached equilibrium"? What does this statement mean regarding the forward and reverse reaction rates? What does this statement mean regarding the amounts or concentrations of the reactants and the products? |

What is meant when a reaction is described as “having reached equilibrium"? What does this statement mean regarding the forward and reverse reaction rates? What does this statement mean regarding the amounts or concentrations of the reactants and the products? |

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

Related questions

Q: The concentration of reactant is very important for a chemical reaction.

A: Rate law is an expression thwt determines the speed of a reaction. It depends upon concentrations of…

Q: Determine whether the following statements are true or false. If a statement is false, explain why.…

A: The reaction at equilibrium is the chemical reaction in which the reactants and products attains a…

Q: 2H₂S(g) = 2H₂(g) + S₂(g) A 6.82 g sample of H2S gas is heated in a 0.500 L rigid container. At…

Q: For an endothermic reaction in equilibrium,an increase in temperature makes the reaction go in the…

A: According to Le-chatlier principle if we change volume , temperature and pressure of the reaction…

Q: For the reaction N₂O4 (g) 2 NO₂ (g), determine the equilibrium constant when only an initial amount…

A: N2O4(g)↔2NO2(g) for the given equilibrium reaction K = [NO2]2/[ N2O4] where K =…

Q: As we continue to explore equilibrium, it is important that we look at LeChatelier's Principle. This…

A: Your argument is true. As per LeChatelier's Principles if we remove the product from reaction…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: What are reactions at equilibrium

A: In this questions, we will discuss about equilibrium reactions. You can see details explanations…

Q: For the equilibrium reaction: 2 NOCl(g) 2 NO(g) + Cl2(g) 3.00 mol NOCl was placed in an otherwise…

Q: Discuss a scenario that you have experienced personally that manifests chemical equilibrium.

A: The answer is attached below-

Q: What happens to a reaction at equilibrium when there is an abundance of sodium carbonate and calcium…

A: In a chemical reaction at equilibrium, the concentrations of reactants and products remain constant…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

A: The detailed solution of the above question is given below;Explanation:

Q: Suppose a 250. ml. flask is filled with 1.7 mol of H, and 1.2 mol of NH,. This reaction becomes…

A: Chemical equilibrium is defined as the speed at which rate of reaction occurs.

Q: Suppose a 250. mL flask is filled with 1.6 mol of SO, and 1.1 mol of SO,: This reaction becomes…

A: The volume of 1000 mL is equal to 1.0 L. The molarity of the SO2 is calculated as shown below.…

Q: Observe things around you on a day-to-day basis, and identify where chemical equilibrium principles…

A: Chemical equilibrium is an essential concept in understanding many natural and industrial processes.…

Q: Consider the equilibrium H2(g) + I2(g) double arrow 2HI(g), what will happen if total volume…

A: Given reaction is : H2 (g) + I2 (g) <--------------> HI (g) What will happen if total volume…

Q: scribes the behavior of the system if POB is added to the container? The reverse reaction will…

A: According to Le-chatlier principle if we change volume , temperature and pressure of the reaction…

Q: The law of chemical equilibrium states that “at equilibrium there is a constant ratio between the…

A: Equilibrium is defined as the state where the rate of the forward reaction and the reverse reaction…

Q: moles

Q: For the reaction: H₂O(l) 2NH3(g) + CO₂(g) = (NH₂)2CO(s) + AH = - 330 kJ

A: Answer: According to Le-Chatalier's principle, on changing any parameter of the system that is in…

Q: an exothermic reactionr

A: Formation of ammonia is a exothermic process that means heat is librated hence according to…

Q: N,(g)+3H,(g)- 12NH,(g) Complete the table below, so that it lists the initial molarity of each…

A: Molarity is defined as number of solute present in 1000 ml of solution . Mole=…

Q: Describe the forward and reverse reactions of constant equilibrium?

A: Forward reactions favor the formation of products and the reverse reaction favors the formation of…

Q: Consider the following equilibrium: NF3 (g) + F2 (g) = NF5 (g) AH = -560 kJ/mol According to the Le…

A: To solve this problem use le chatelier's principle.

Q: For an endothermic reaction in equilibrium,an increase in temperature makes the reaction go in…

A: Endothermic reaction is chemical reaction which requires heat or energy to complete the reaction .

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: Describe the concentration of reactants and products at equilibrium.

A: Types of reactions: Based on extent of completion reactions are two types 1. Irreversible…

Q: In general, for a system at equilibrium, indicate the direction the equilibrium will shift for the…

A: Given: The concentration of one or more of the reactants is decreased.

Q: If 2.4 mol of HCl was placed in a 0.8 L container and allowed to reach equilibrium, what would the…

A: It is given that 2.4 mol of HCl undergoes a reaction to give H2 and Cl2. For that reaction…

Q: Part D decreasing the volume of the container The equilibrium concentration of NH, will decrease.…

A: Le Chatelier's principle: This principle is used to predict the effect of a change in conditions on…

Q: Dynamic equilibrium means that at equilibrium The reverse reaction stops The forward reaction stops…

A: At equilibrium both forward and backward takes place and also the concentration of product and…

Q: Consider the reaction. PCI, (g) PC13(g) + Cl₂(g) Kc = 0.0420 The concentrations of the products at…

Q: True or False? 1. The concentration of reactants and products at equilibrium can be any random…

A: No this statement is false .

Q: Which of the following conditions characterizes a system in a state of chemical equilibrium? A. The…

Q: Why does the equilibrium of a system shift when the pressure is decreased? O To maximize the stress…

A: According to the Le chatelier's principal, " when a system is already…

Q: What does Le Chatelier's principle state? • A reaction can proceed both forward and backward in a…

A: Le Chatelier principle states that equilibrium adjusts the forward and backward reactions in such a…

Q: Which of the following correctly describes chemical equilibrium? A. Concentrations of products…

A: The Chemical equilibrium represents a dynamic balance in a chemical system, where the rates of the…

Q: Explain Le Chatelier’s principle. How can this principle help us maximize the yield of reactions?…

Q: Explain a condition that could be changed in a system that would increase the amounts of products at…

A: The condition that could be changed in a system to increase the amounts of products at equlibrium…

Q: If the equilibrium constant for an equilibrium system has decreased because of a "stress", how have…

Q: An equilibrium mixture of PCI, (g), PCI, (g), and Cl, (g) has partial pressures of 217.0 Torr, 13.2…

Q: What is meant by dynamic equilibrium? Include comparison of the rates of forward and reverse…

A: Equilibrium exists in the reactions only if the reaction is reversible in nature. At the state of…

Q: Look at the reaction below and state which direction the reaction would shift: A closed container of…

Question

1. What is meant when a reaction is described as “having reached equilibrium"? What does this statement
mean regarding the forward and reverse reaction rates? What does this statement mean regarding the
amounts or concentrations of the reactants and the products?
2. In your own words, explain the "Law of Mass Action".

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Look at the reaction below and state which direction the reaction would shift: A closed container of water and its vapor at equilibrium. Vapor is added to the system. Water + Energy <=> Vapor Explain your reasoning.
6. The concentration of reactans and the concentration of the products at equilibrium A. If the first quantity is less than the second quantityB. If the first quantity is greater than second quantityC. If the two quantities are equalD. If the two quantities cannot be compared
Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.1 mol of NH,. This reaction becomes possible: N, (g) +3H,(g) =2NH, (g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. olo Ar N2 H, NH, initial change equilibrium 미
What can be said about the magnitude of the equilibrium constant in a reaction whose equilibrium lies far to the right? To the left?
Increasing the concentration of the reactants will slow down the reaction. O true O false
is a substance that increases the rate of reaction but has no effect on the equilibrium composition of a reaction mixture. A Moving to another question will save this response.
Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed? a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases
1. The reaction shown below is carried out at various temperatures and the value of Kc determined. Draw particulate representations that show the relative amounts of each reactant and product that would roughly correspond to the value of K. Legend = PC13 = Cl₂ ∞ = = PC15 PC13 (g) + Cl2 (g) = PC15 (g) Magnitude of K Particulate diagram of equilibrium mixture 1 x 10 -3 1 x 105
Define equilibrium in terms of a)reaction rates -Forward reaction rate = reverse reaction rate b)changes in observable properties -There are no observable changes c)energy and energy changes -Energy has become stable (no longer giving off or taking in heat)
Decide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction. d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.
What happens to a chemical system at equilibrium when that equilibrium is disturbed?
In general, for a system at equilibrium, indicate the direction the equilibrium will shift for the following change. The concentration of one or more of the products is increased.