Need solution urgently paternceConsider the reactionPela) - 2P(9)where K,1.00 x 10 at 1325 K. In an experiment where Pa(9) is placed into a container at 1125 K, the equilibrium misture of Palo) and P(9) has a total pressure of 2.71atn. Calculate the equilrum pressures of Pelg) and P(9) Calculate the fraction (by moles) of Pale) that has dissociated to reach egulibriumEquibrum pressure f Pale)atmfertquibriuni pressure of P(9)atmFraction of P.) doatedIprSubmit AnrTry Aner Versionaes remainingfar

Answered: Image /qna-images/answer/dcc60e7c-eab6-442c-aa46-d31eb2971b79.jpg

paternce Consider the reaction Pela) - 2P(9) where K,1.00 x 10 at 1325 K. In an experiment where Pa(9) is placed into a container at 1125 K, the equilibrium misture of Palo) and P(9) has a total pressure of 2.71 atn. Calculate the equlbrum pressures of Pelg) and Py(9) Calculate the fraction (by moles) of Pale) that has dissociated to reach egulibrium tqulbrium pressure of Pale) atm fer touibriuni pressure of P(9) atm Fraction of P.() dioated pr Submit A r Try Aner Version eams remaining

paternce Consider the reaction Pela) - 2P(9) where K,1.00 x 10 at 1325 K. In an experiment where Pa(9) is placed into a container at 1125 K, the equilibrium misture of Palo) and P(9) has a total pressure of 2.71 atn. Calculate the equlbrum pressures of Pelg) and Py(9) Calculate the fraction (by moles) of Pale) that has dissociated to reach egulibrium tqulbrium pressure of Pale) atm fer touibriuni pressure of P(9) atm Fraction of P.() dioated pr Submit A r Try Aner Version eams remaining

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...

See similar textbooks

Similar questions

Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
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?
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
For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr, respectively, were allowed to react at 300. K. At equilibrium the total pressure was 110.5 torr. The reaction is 2NO(g)+Br2(g)2NOBr(g) a. Calculate the value of Kp. b. What would be the partial pressures of all species if NO and Br2, both at an initial partial pressure of 0.30 atm, were allowed to come to equilibrium at this temperature?
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?
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?