Answered: You place 1.74 mol of pure SO3 in an…

You place 1.74 mol of pure SO3 in an 8.0-L flask at 1150 K. At equilibrium, 0.38 mol of O2 has been formed. Calculate K. for the reaction at 1150 K 2 SO3 (g) 2 2 SO2(g) + O2(g) K.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

While ethanol (CH3CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 25 L tank with 1.9 mol of ethylene gas and 5.7 mol of water vapor. When the mixture has come to equilibrium he determines that it contains 0.97 mol of ethylene gas and 4.77 mol of water vapor. The engineer then adds another 0.95 mol of ethylene, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. mol x10 X
Be sure to answer all parts. The equilibrium constant K, for the reaction I(g) 5 21(g) is 3.75 x 10 at 726°C. Calculate K, and Kp for the equilibrium 21(g) S1(g) at the same temperature. K.= X 10 %3D (Enter your answer in scientific notation.) Kp = %3D
Initially, 1.50 M of ammonia (NH3) were placed in an empty container without any other gases at 789K. It started to decompose according to the chemical equation below: 2 NH3(g) = N₂(g) + 3 H₂(g) After equilibrium was established, it was found that there are 0.055 M of ammonia left in the same vessel. What is the equilibrium constant, Kc, for this reaction at 789 K? 3.5 28 9.8 x 103 2.4 x 10³ O4.8 x 104
Consider the following reaction where K. = 10.5 at 350 K: 2 CH;Cl2 (g)=CH4 (g)+ CCI4 (g) A reaction mixture was found to contain 1.10x10-2 moles of CH,Cl, (g), 4.63×10-2 moles of CH4 (g), and 3.70×10² moles of CCl (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: v 1. In order to reach equilibrium CH,Cl,(g) must be produced. v 2. In order to reach equilibrium K, must decrease v 3. In order to reach equilibrium CH, must be consumed. v 4. Qc is greater than K. 5. The reaction is at equilibrium. No further reaction will occur. T
For the reaction PCL5 (g) = PCl3 (g) + Cl₂ (g) at equilibrium, Kp = 321. The equilibrium partial pressures of PCl3 and Cl₂ are 1.00E0 atm and 4.50E0 atm, respectively. What is the equilibrium partial pressure of PCl5?
The equilibrium constant, Kc, for the following reaction is 83.3 at 500 K.PCl3(g) + Cl2(g) PCl5(g)Calculate the equilibrium concentrations of reactant and products when 0.271 moles of PCl3 and 0.271 moles of Cl2 are introduced into a 1.00 L vessel at 500 K.
While ethanol (CH3CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 500. mL flask with 0.77 atm of ethylene gas and 0.98 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.34 atm of ethylene gas and 0.55 atm of water vapor. The engineer then adds another 0.19 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm
The equilibrium constant, Kc, for the following reaction is 57.6 at 277 K. 2CH₂Cl₂ (g) CH4 (9) + CCl4 (9) When a sufficiently large sample of CH₂Cl₂ (g) is introduced into an evacuated vessel at 277 K, the equilibrium concentration of CC14 (g) is found to be 0.383 M. Calculate the concentration of CH₂Cl₂ in the equilibrium mixture. [CH₂Cl₂] = M
For the equilibrium N2(g)+O2 <-->2NO(g), Kp = 0.0017 at 2300 K. At a given point, the partial pressures of the gases are PN2=PO2 = 0.660 atm and PNO= 0.0272atm. Which statment below is true? a. Q < K, so the reaction will continue to make more products. b. Q > K, so the reaction will consume products to make more reactants. c. Q = K, so the system is at equilibrium. d. The value of K will decrease until it is equal to Q. Show your work:
Consider the equilibrium system described by the chemical reaction below. If the partial pressures at equilibrium of NO, Cl2, and NOCI are 0.095 atm, 0.171 atm, and 0.28 atm, respectively, in a reaction vessel of 7.00 L at 500 K, what is the value of Kp for this reaction? 2 NO(g) + Cl2(g) = 2 NOCI(g)
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
Please don't provide handwritten solution ....