4 moles of PCls are placed in a 5.0 L container. Dissociation takes place accordingto the equationPCls(g)PCl;(g) + Cl½(g).At equilibrium, 0.40 mol of Cl, are present. Calculate the equilibrium constant (K.)theforthisreactionunderconditionsofthisexperiment.0.30.0200.00880.0880.03

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Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.40QE

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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
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
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?
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4 moles of PCls are placed in a 5.0 L container. Dissociation takes place according to the equation PCls(g) PCl;(g) + Cl½(g). At equilibrium, 0.40 mol of Cl, are present. Calculate the equilibrium constant (K.) the for this reaction under conditions of this experiment. 0.3 0.020 0.0088 0.088 0.03