4. For the equilibrium: 2 BrCL (g) Br2 (g) CI2 (g) at 205 °C, the equilibrium constant, Kc, is 0.143. If 1.34 moles each of Br2 (g) and Cl2 (g) are introduced in a container which has a volume of 11.0 liters and allowed to reach equilibrium at 205 °C, what would be the concentrations of Br2 (g), Cl2 (g), and BrCl (g) at equilibrium? Setup:

4. For the equilibrium: 2 BrCL (g) Br2 (g) CI2 (g) at 205 °C, the equilibrium constant, Kc, is 0.143. If 1.34 moles each of Br2 (g) and Cl2 (g) are introduced in a container which has a volume of 11.0 liters and allowed to reach equilibrium at 205 °C, what would be the concentrations of Br2 (g), Cl2 (g), and BrCl (g) at equilibrium? Setup:

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.98PAE

See similar textbooks

Related questions

Q: Determine whether the following statements are true or false. Correct the false statements. The…

Q: True or false? a reversible reaction has reached equilibrium when the concentration of the…

A: A chemical reaction is said to have reached equilibrium when the rate of formation of products from…

Q: Which of the following causes the equilibrium concentrations of the products of an equilibrium to…

A: When a reaction proceeds, the reactants convert to products. The amounts of reactants decrease with…

Q: Explain chemical equilibrium in terms of the reactions rate of the forward and the reverse reaction.

A: For any chemical reaction in which reactants are going towards the formation of products or vice…

Q: Steam reforming of methane ( CH, ) produces "synthesis gas," a mixture of carbon monoxide gas and…

Q: Solid iron (ii) oxide and carbon monoxide gas are in equilibrium with solid iron and carbon dioxide…

A: Reaction between Solid iron(ll) Oxide and Carbon monoxide gas produce the solid iron and carbon…

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: What is the correct equilibrium constant expression for the balanced reaction shown below? NO(g) +…

Q: Which factors must be equal in a reversible chemical reaction at equilibrium? * The concentrations…

A: The state of the system in which the measurable properties of the system such as concentration,…

Q: What happens to a reaction at equilibrium when more reactants are added to the system? The reaction…

A: According to Le Chateliar principle if a system is in equilibrium is subjected to change of…

Q: So what are there equilibrium constant values?

A: In this question, what are there equilibrium constant values in the preceding question.

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Given that : We have to calculate the moles of hydrogen after equilibrium is reached for the second…

Q: Consider the following equilibrium: PCI5(g) + PCI3(g) + Cl2(g) A 1.00 L flask contains 0.0200 mol…

Q: Which of the following explains the term "dynamic" as applied to chemical equilibrium? Group of…

A: A reversible chemical reaction can move in either forward or backward direction. The stage of a…

Q: Explain Le Chatelier's principle as it relates to chemical equilibrium. Describe the types of…

A: Le Chatelier's principle states that if an equilibrium reaction is disturbed by changing pressure,…

Q: Select all the TRUE statements about chemical equilibrium. At equilibrium the rates of the forward…

A: The objective of the question is to identify the correct statements about chemical equilibrium.

Q: Select all of the true statements regarding chemical equilibrium. The concentrations of reactants…

Q: Increasing the concentration of the reactants will slow down the reaction. O true O false

A: During a reaction, reactant is converted into product.

Q: Define equilibrium in terms of a)reaction rates -Forward reaction rate = reverse reaction rate…

A: Eqilibrium can be defined in terms of reaction rate, change in observable properties, energy and…

Q: The addition of a catalyst will change the composition of the equilibrium mixture. True False

A: we need to tell if the given statement is correct or not

Q: Which of the following statements concerning equilibrium is not true? a The equilibrium…

Q: When a system is at equilibrium: the reaction rate of the forward reaction is small compared to the…

A: The system is at equilibrium, the reaction rate of the forward reaction is equal to the rate of the…

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

Q: The graph below shows the concentration of reactants and products in a chemical reaction that…

A: Given:- We have to explain the nature of graph which is representing equilibrium .

Q: Which of the following is/are true concerning a chemical reaction at equilibrium? 1. The system…

A: For the reversible reaction the condition where the rates of forward and reverse reactions become…

Question

Write all equilibrium equations Write all equilibrium concentrations Write all equilibrium expressions

4.
For the equilibrium:
2 BIGL (g)
Br2 (g) CIZ (g)
at 205 °C, the equilibrium constant, Kc, is 0.143. If 1.34 moles each of Br2 (g) and Cl2 (g) are introduced in
a container which has a volume of 11.0 liters and allowed to reach equilibrium at 205 °C, what would be the
concentrations of Br2 (g), Cl2 (g), and BrCl (g) at equilibrium?
Setup:

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 with 2 images

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

Consider the following reactions at some temperature: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105 2NO(g)N2(g)+O2(g)K=11031 For each reaction, assume some quantities of the reactants were placed in separate containers and allowed to come to equilibrium. Describe the relative amounts of reactants and products that would be present at equilibrium. At equilibrium, which is faster, the forward or reverse reaction in each case?
Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species. (b) The volume of the container is decreased to 4.5 L and the system allowed to return to equilibrium. Calculate the new equilibrium concentrations. (Hint: The calculation will be easier if you view this as a new problem with 0.5 mol of COBr2 transferred to a 4.5-L flask.) (c) What is the effect of decreasing the container volume from 9.50 L to 4.50 L?
Consider the equilibrium N2(g)+O2(g)2NO(g) At 2300 K the equilibrium constant Kc = 1.7 103. If 0.15 mol NO(g) is placed into an empty, sealed 10.0-L flask and heated to 2300 K, calculate the equilibrium concentrations of all three substances at this temperature.
For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture consists of all three gases with the following partial pressures: PPCl5=0.026atm,PPCl3=0.65atmPPCl2=0.33atm (a) Is the system at equilibrium? Explain. (b) If the system is not at equilibrium, in which direction will the system move to reach equilibrium?
Consider the following reaction at 1000 C: NO(g)+12 Cl2(g)NOCl(g) (a) Write an equilibrium constant expression for the reaction and call it K'. (b) Write an equilibrium constant expression for the decomposition of NOCl to produce one mole of chlorine gas. Call the constant K. (c) Relate K' and K.
Molecular bromine, Br2, dissociates at elevated temperatures into bromine atoms, Br. Br2(g)2Br(g) A 3.000-L flask initially contains pure molecular bromine. The temperature is then raised to 1600 K. If the total pressure of this equilibrium mixture at this elevated temperature is 1.000 atm, what are the total moles of gas in the container? A spectroscopic analysis of this mixture showed that it contained 1.395 g of Br atoms. What is the partial pressure of Br? What is Kp for the dissociation of molecular bromine to bromine atoms?
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
A mixture of 0.0565 mol phosphorus pentachloride, PCl5, and 0.0800 mol helium gas, He, was placed in a 1.000-L flask and heated to 250.0C. The phosphorus pentachloride decomposes at this temperature to give phosphorus trichloride, PCl3, and chlorine gas, Cl2. The helium gas is inert. PCl5(g)PCl3(g)+Cl2(g) What is the partial pressure of helium in this equilibrium mixture at 250.0C? At equilibrium, the total pressure is found to be 6.505 atm. What is Kc for the dissociation of PCl5?
A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.
5.19. Assume that a reaction exists such that equilibrium occurs when the partial pressures of the reactants and products are all . If the volume of the system were doubled, all of the partial pressures would be . Would the system still be at equilibrium? Why or Why not?
Mustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer