4. [Review Toples)References]Use the References to access important values if needed for this question.The equilibrium constant, K, for the following reaction is 1.20x102 at 500 K.PCI5(g) PCI3(9) + Clz(g)An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.262 M PCIs, 5.61x102 M PCI, and5.61x102 M CI,. What will be the concentrations of the three gases once equilibrium has been reestablished, if4.78x102 mol of Cl2(g) is added to the flask?[PCIg) -M.[PCI3)=M.(Cl2)M.%3DSubmit AnswerRetry Entire GroupNo more group attempts remain(Previous

Answer: According to Le-chatalier's principle on adding Cl2 for the given system at equilibrium, it…

The equilibrium constant, K, for the following reaction is 1.20x102 at 500 K. PCI,(9) PCly(9) + Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.262 M PCI,, 5.61x102 M PCI, and 5.61x102 M Clz2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.78x102 mol of Cl2(9) is added to the flask? (PCIs) - M. (PCI,)- M. (Cl2) M.

The equilibrium constant, K, for the following reaction is 1.20x102 at 500 K. PCI,(9) PCly(9) + Cl2(g) An equilibrium mixture of the three gases in a 1.00 L flask at 500 K contains 0.262 M PCI,, 5.61x102 M PCI, and 5.61x102 M Clz2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 4.78x102 mol of Cl2(9) is added to the flask? (PCIs) - M. (PCI,)- M. (Cl2) M.

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

Similar questions

Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
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?
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
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.
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open 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?
The following two diagrams represent the composition of an equilibrium mixture for the reaction A2 + B2 2AB at two different temperatures. Based on the diagrams, is the chemical reaction endothermic or exothermic? Explain your answer using Le Chteliers principle. (A atoms are red and B atoms are green in the diagrams.)