Iodine and bromine reactto give iodinemonobromide, IBr.I2 (g) + Br2 (g)= 2IBr(g)What is the equilibriumcomposition of a mixtureat 139°C that initiallycontained2.10 x 10-3 mol eachof iodine and bromine ina 5.00 L vessel? Theequilibrium constantK. for this reaction at139°C is 95.7.[I2]M[Br2]M[IBr] =M

Answered: Image /qna-images/answer/fb984478-b81d-465b-9e7e-1842877a5177.jpg

Iodine and bromine react to give iodine monobromide, IBr. I2 (g) + Br2 (g)= 2IB1(. What is the equilibrium composition of a mixture at 139°C that initially contained 2.10 x 10- mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant K. for this reaction at 139°C is 95.7.

Iodine and bromine react to give iodine monobromide, IBr. I2 (g) + Br2 (g)= 2IB1(. What is the equilibrium composition of a mixture at 139°C that initially contained 2.10 x 10- mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant K. for this reaction at 139°C is 95.7.

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 12.34PAE: 1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was...

See similar textbooks

Related questions

Q: Be sure to answer all parts. The equilibrium constant (K) for the formation of nitrosyl chloride, an…

A: Given that - For the following reaction - 2NO(g) + Cl2(g) -----> 2NOCl(g) Kc = 3×104 and…

Q: Sulfur trioxide, used to manufacture sulfuric acid, is obtained commercially from sulfur dioxide.…

Q: Consider the reaction:SO2Cl2( g) <-------->SO2( g) + Cl2( g) Kp = 2.91 * 103 at 298 KIn a…

Q: Consider the equilibrium system described by the chemical reaction below, which has a value of Kc…

A: Given data,Kc=1.79Initial Concentration of H2S=0.05MInitial concentration of SO2=0.05M

Q: The following acid-base reaction occurs spontaneously in the gas phase: NH,(g) + HCI(g) = NH,C(s)…

Q: The equilibrium constant, K, for the following reaction is 9.52x102 at 350 K. CH4 (g) + CCI, (g) 2…

Q: Be sure to answer all parts. The equilibrium constant (K) for the formation of nitrosyl chloride, an…

Q: The following equilibrium was studied by analyzing the equilibrium mixture for the amount of HCl…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: The equilibrium constant K, for the reaction H2(g) + Br,(g) - 2HBr(g) is 2.18 x 10 at 730°C.…

Q: For the reaction 2 A (g) + B (g) = C(g) + D(s) AH = - 33.0 kJ 1. Initially in a 5.0 L flask at 75°C,…

A: 1. Since, solids do not exert any pressure, so D will not have any pressure. Thus, ICE table for the…

Q: A 0.090 mol of gaseous dinitrogen tetroxide, N2O4 dissociates into nitrogen dioxide, NO2 at 383 K.…

A: According to le chatelier's principle if heat is given to the system, the the reaction will go…

Q: Consider the reaction N,(g) + 0,(g) =2NO(g) that has an equilibrium constant, K, fof 4.10 x 10 at…

Q: E. Nitric oxide, NO, is formed in automobile exhaust by the reaction of N2 and 02 in air. N2 (g) +…

A: Given: Moles of N2 =1.00 molMoles of O2 =1.00 molVolume of the container = 2.00 LKc = 0.0025 at…

Q: At a given temperature, the equilibrium constant for a certainreaction is 1 * 1020. Does this…

A: The given value of equilibrium constant is, Keq = 1 ×1020 To find: If this equilibrium favor…

Q: Consider the equilibrium: El Conversat NO + 02 > NO2 for which the equilibrium constant K = 511 at…

A: Given: The reaction is as follows: 2NO + O2 ------------> 2NO2 The K= 511 . The moles of…

Q: Some SO2 is placed in a flask and heated with oxygen to 600°C, at whichpoint K2 = 9.5. At…

A: Partial pressure can be understood as the pressure of the individual gas in a mixture. According to…

Q: The first step in the industrial synthesis of hydrogen is the reaction of steam and methane to give…

Q: The equilibrium constant (Kc) for the reaction PC13 (g) + Cl₂ (g) → PC1, (g) equals 49 at 230°C. If…

Q: Some PCI5 is allowed to dissociate into PCI, and Cl, at 523 K. At equilibrium, [PCl3] = 0.129 M, and…

Q: At 1285° C the equilibrium constant for the reaction Br2 (g) 2 Br (g) is K. = 1.04 x 10 3. A 0.898-L…

A: Kc = [Br]^2/[Br2] Given mass of Br2 = 0.918 g Kc =0.00104 Concentration = moles /volume (in L)…

Q: A chemist Is studying the following equilibirum, which has the glven equilibriiim constant at a…

A: Given: Value of Kp= 3 x 10-9Balanced Reaction is:2CH4 (g) ⇌ C2H4(g) + 3H3(g) Initial pressure of…

Q: 3. The following equilibrium process has been studied at 458°C. NazCO3 (s) + SO2 (g) +02 (g) )…

Q: 3. Nitric oxide, NO, is formed in automobile exhaust by the reaction of N2 and 02 in air. N2 (g) +…

Q: The decomposition of ammonia is: 2 NH3 (g) N2 (g) + 3 H2 (g). If K, is 2.8 x 102, what is the…

A: Consider a general reaction : aA + bB <------> cC + dD The equilibrium constant, Kp is…

Q: For the reaction N2 (g) + O2(g) ↔ 2NO (g), Kc = 0.10 at 2000oC. At a point during the…

A: Equilibrium constant is defined as ratio of concentration of to the concentration of reaction

Q: Consider the reaction: H2(g) + Br2(g) --> 2HBr(g) ΔH˚ = -103.8 kJ/mol In a particular experiment,…

Q: Consider the following reaction: PClg(g) PCl,(g)+ Ch(g) If 2.82x10 moles of PClg(g), 0.571l moles of…

A: Given, a equilibrium chemical reaction,PCl5(g)⇋PCl3(g)+Cl2(g) and, at equilibrium the number of…

Q: The equilibrium constant for the following reaction is 10.5 at 350K. 2CH,Cl½(g) CH,(g) + CCI4(g) If…

A: Equilibrium constant is defined as the ratio of concentration of products to concentration of…

Q: Be sure to answer all parts.The equilibrium constant (K) for the formation of nitrosyl chloride, an…

Q: Consider the reaction, which takes place at a certain elevated temperature CO(g)+NH3(g)⇌HCONH2(g)…

Q: Some PClg is allowed to dissociate into PCl, and Cl2 at 523 K. At equilibrium, [PCI3] = 0.129 M, and…

A: Given reaction is : PCl5 (g) <------------> PCl3 (g) + Cl2 (g) Initial concentration of PCl5…

Q: Consider the following reaction: 2HI(g) H2(g) + I2(g) If 2.77 moles of HI(g), 0.315 moles of H2,…

A: The equilibrium reaction taking place is given as, => 2 HI (g) ↔ H2 (g) + I2 (g) Given: Volume of…

Q: B. The decomposition of dinitrogen tetroxide gas forms nitrogen dioxide gas. What is the value of K,…

Q: what will be the equilibrium concentration of BrCl?

Q: For the reaction 2 H2O (l) ⇌ 2H2 (g) + O2 (g), the equilibrium expression is:

A: Equilibrium constant: At equilibrium the ratio of products to reactants has a constant value. It is…

Q: For the reaction I2(g) + Br2(g) ⇔ 2IBr(g), Kc = 280 at 150o C. Suppose that 0.500 mol IBr in a 1.00…

A: The equilibrium constant for a chemical reaction can be given as follows: aA+bB→cC+dD…

Q: Iodine Chloride decomposes at high temperatures to iodine and chlorine gases. 2ICl(g) I2(g) +…

Q: Phosphorus pentachloride, PCl5, decomposes when heated. PCl5 (g) ↔ PCl3 (g) + Cl2 (g) If the…

A: A chemical reaction which proceeds in both directions is called reversible reaction. Chemical…

Q: The decomposition of ammonia is: 2 NH3(g) - N2(g) + 3 H2(g). If K, is 1.5 x 103 at 400°C, what is…

Q: Be sure to answer all parts. The equilibrium constant (K) for the formation of nitrosyl chloride, an…

A: Given-> 2NO(g) + Cl2(g) ---> 2NOCl(g) Kc= 5×106 Mole of NO = 9.30 × 10-2 Mole of Cl2 = 1.60 ×…

Q: 1. During one step in the synthesis of nitric acid, nitrogen dioxide (NO2) is in equilibrium with…

A: We have to predict the equilibrium constant.

Q: For the following chemical equilibrium: N2(g) + O2(g) 2NO(g), the equilibrium constant (Kp) was…

Q: Consider the reaction 2 H2(g) + O2(g) 2 H2O(g). Suppose that initially [H2] = 1.0 M and [O2] =…

A: First to draw ICE table then to find equilibrium concentration of all. Then using equilibrium…

Q: Isopropyl alcohol can dissociate into acetone and hydrogen: (CH3),CHOH(g) 2 (CH;),CO(g) + H2(g) At…

A: Given data: Equilibrium constant : Kp =0.444 Tempreature : T = 179 oC mass of isopropyl alcohol…

Q: Consider the following equilibrium system at 355 K. 2NOBr(g) -----> 2NO(g)+Br2(g). If an equilibrium…

A: [NOBr] = 3.21 x 10-2 M [NO] = 2.01 x 10-2 M [Br2] = 3.98 x 10-2 M Keq = ?

Q: Consider the following equilibrium: C2H6(g) + C5H12(g) CH4(g) + C6H14(g); Kp = 9.57 at 500 K…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: You place 0.600 mol of nitrogen, N2, and 1.800 mol of hydrogen, H2, into a reaction vessel at 450°C…

Q: Phosphorus pentachloride gas decomposes to phosphorus trichloride gas and chlorine gas at 250…

A: If a reaction is already at equilibrium and we add some reactant to it, then the concentration of…

Question

Iodine and bromine react
to give iodine
monobromide, IBr.
I2 (g) + Br2 (g)= 2IBr(g)
What is the equilibrium
composition of a mixture
at 139°C that initially
contained
2.10 x 10-3 mol each
of iodine and bromine in
a 5.00 L vessel? The
equilibrium constant
K. for this reaction at
139°C is 95.7.
[I2]
M
[Br2]
M
[IBr] =
M

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

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps with 5 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

At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
Butane exists as two isomers, n -butane and isobutane. Kp=2.5 at 25 C What is the pressure of isobutane in a container of the two isomers at equilibrium with a total pressure of 1.22 am?
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
At 25C. Kp = 5.3 105 for the reaction N2(g)+3H2(g)2NH3(g) When a certain partial pressure of NH3(g) is put into an otherwise empty rigid vessel at 25C, equilibrium is reached when 50.0% of the original ammonia has decomposed. What was the original partial pressure of ammonia before any decomposition occurred?
A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure at equilibrium is 40% greater than it was originally, when only I2 was present. What is K for this reaction at that 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?
Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S produced. Sb2S3(s)+3H2(g)2Sb(s)+3H2S(g) A vessel whose volume was 2.50 L was filled with 0.0100 mol of antimony(III) sulfide, Sb2S3, and 0.0100 mol H2. After the mixture came to equilibrium in the closed vessel at 440C, the gaseous mixture was removed, and the hydrogen sulfide was dissolved in water. Sufficient lead(II) ion was added to react completely with the H2S to precipitate lead(II) sulfide, PbS. If 1.029 g PbS was obtained, what is the value of Kc at 440C?
At 2000 K, experiments show that the equilibrium constant for the formation of water is 1.6 1010. 2H2(g) + O2(g) 2H2O(g) Calculate the equilibrium constant at the same temperature for H2(g)+12O2(g) H2O(g)