When the below reaction occurs at 55°C, the respective pressures of N2O4 (g) and NO2 (g) at2.equilibrium are 0.212 atm and 0.254 atm. Calculate both equilibrium constants, Kp and KçN2O4 (g)2 NO2 (g)

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

Answered: When the below reaction occurs at 55°C,…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 40E: The equilibrium constant is 0.0900 at 25C for the reaction H2O(g)+Cl2O(g)2HOCl(g) For which of the...

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The equilibrium constant is 0.0900 at 25C for the reaction H2O(g)+Cl2O(g)2HOCl(g) For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift? a. PH2O=1.00atm,PCl2O=1.00atm,PHOCl=1.00atm b. PH2O=200.torr,PCl2O=49.8torr,PHOCl=21.0torr c. PH2O=296torr,PCl2O=15.0torr,PHOCl=20.0torr
The equilibrium constant is 0.0900 at 25C for the reaction H2O(g)+Cl2O(g)2HOCl(g) For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift? a.PH2O=1.00atm,PCI2O=1.00atm,PHOCI=1.00atm b.PH2O=200.torr,PCI2O=49.8torr,PHOCI=21.0torr c. PH2O=296torr,PCI2O=15.0torr,PHOCI=20.0torr
At a certain temperature, nitrogen and oxygen gases combine to form nitrogen oxide gas. N2(g)+O2(g)2NO(g)When equilibrium is established, the partial pressures of the gases are: PN2=1.200atm,PO2=0.800atm,PNO=0.0220atm. (a) Calculate K at the temperature of the reaction. (b) After equilibrium is reached, more oxygen is added to make its partial pressure 1.200 atm. Calculate the partial pressure of all gases when equilibrium is reestablished.
. 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?
Calculate K for the formation of methyl alcohol at 100C: CO(g)+2H2(g)CH3OH(g) given that at equilibrium, the partial pressures of the gases are PCO=0.814 atm, PH2=0.274 atm, and PCH3OH=0.0512 atm.
Consider the decomposition at 25C of one mole of NOBr gas into NO and Br2 gases. At equilibrium, the concentrations of NOBr, NO, and Br2 gases are 0.0162 M, 0.0011 M, and 0.072 M, respectively. (a) Write a balanced equation for the reaction. (b) Calculate K for the reaction at 25C. (Note that the gases need to be expressed as pressure in atm.)
Consider the equilibrium H2(g)+S(s)H2S(g)When this system is at equilibrium at 25C in a 2.00-L container, 0.120 mol of H2, 0.034 mol of H2S, and 0.4000 mol of S are present. When the temperature is increased to 35C, the partial pressure of H2 increases to 1.56 atm. (a) What is K for the reaction at 25C? (b) What is K for the reaction at 35C?
Explain why an equilibrium between Br2(l) and Br2(g) would not be established if the container were not a closed vessel shown in Figure 13.5.
A piece of gold (10.0 g, CAu = 0.129 J/g K) is heated to 100.0 C. A piece of copper (also 10.0 g, CCu = 0.385 J/g K) is chilled in an ice bath to 0 C. Both pieces of metal are placed in a beaker containing 150. g H2O at 20 C. Will the temperature of the water be greater than or less than 20 C when thermal equilibrium is reached? Calculate the final temperature.
Kp for the following reaction is 0.16 at 25 C: 2 NOBr(g) 2 NO(g) + Br2(g) The enthalpy change for the reaction at standard conditions is + 16.3 kJ/mol-rxn. Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more Br2(g) (b) removing some NOBr(g) (c) decreasing the temperature (d) increasing the container volume
Determine G for the following reactions. (a) Antimony pentachloride decomposes at 448 C. The reaction is: SbCl5(g)SbCl3(g)+Cl2(g) An equilibrium mixture in a 5.00 L flask at 448 C contains 3.85 g of SbCl5, 9.14 g of SbCl3, and 2.84 g of Cl2. (b) Chlorine molecules dissociate according to this reaction: Cl2(g)2Cl(g) 1.00% of Cl2 molecules dissociate at 975 K and a pressure of 1.00 atm.

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When the below reaction occurs at 55°C, the respective pressures of N2O4 (g) and NO2 (g) at 2. equilibrium are 0.212 atm and 0.254 atm. Calculate both equilibrium constants, Kp and Kç N2O4 (g) 2 NO2 (g)