Answered: 6. A 3.75-L vessel contains 0.444 mol…

6. A 3.75-L vessel contains 0.444 mol SO3 0,632 mol O2, and 2.125 mol SO2 at 230°C in an equilibrium mixture. Calculate the value of Kc at 230°C. (1 2SO2(g) + O2 (g) 2SO3(g) 7

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

The decomposition of HI at low temperature was studied by injecting 2.50 mol of HI into a 10.32-L vessel at 25℃. What is [H2] at equilibrium for the reaction 2HI(g) H2(g) + I2(g); Kc = 1.2610-3 ?
You place 4.57 mol of dinitrogen trioxide, N2O3, into a flask, where it decomposes at 25.0°C and 1.00 atm. N2O3(g) NO2(g) + NO(g) What is the composition of the reaction mixture at equilibrium if it contains 0.59 mol of nitrogen dioxide, NO2?N2O3(g) molNO2(g) molNO(g) mol
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 Keg for the equilibrium below is 7.82 · 10-2 at 510.0 °C. 2Cl, (g) + 2H20 (g) =4HCI (g) + 02 (g) What is the value of Keg at this temperature for the following reaction? Cl2 (g) + H20 (g) = 2HCI (g) + 02 (g) O 0.280 O 0.0376 O 6.12 - 10-3 O 0.150 O 0.0782
While ethanol (CH,CH,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 2.3 atm of ethylene gas and 4.3 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 1.57 atm of ethylene gas and 3.57 atm of water vapor. The engineer then adds another 2.2 atm of water, 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
Consider the following equilibrium:C2H6(g) + C5H12(g) <--> CH4(g) + C6H14(g); Kp = 9.57 at 500 KSuppose 45.4 g each of CH4, C2H6, C5H12, and C6H14 are placed in a 25.0-Lreaction vessel at 500 K. Which way will the reaction go? Why?
Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5⁢(g)⁢↽−−⇀⁢PCl3⁢(g)+Cl2⁢(g) A 13.1 gsample of PCl5 is added to a sealed 1.25 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 48.4% of the PCl5 remains. What is the equilibrium constant, Kc , for the reaction?
For the equilibrium 3H₂(g)+N₂(g) P -0.00239 atm, P," NH₂ -0.763 atm and P 2NH, (g), the equilibrium partial pressures are = 0.921 atm, at 500°C. Calculate Kp.
A student ran the following reaction in the laboratory at 479 K: PCI3(g) + Cl₂(g) =PC15(g) When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she found that the equilibrium partial pressure of PCI5 was 1.12 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining
At a certain temperature, the ?p for the decomposition of H2S is 0.770. H2S(g)↽−−⇀H2(g) + S(g) Initially, only H2S is present at a pressure of 0.268 bar in a closed container. What is the total pressure in the container at equilibrium? Ptotal= bar
While ethanol (CH,CH,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 200. mL flask with 1.7 atm of ethylene gas and 2.2 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.92 atm of ethylene gas and 1.42 atm of water vapor. olo Ar The engineer then adds another 1.1 atm Of water, 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
Consider the following system at equilibrium where AH = 268 kJ and Kc = 5.10 × 10-6, at 548 K. NH4Cl(s) NH3(g) + HCl(9) The production of NH3(g) is favored by (indicate true or false): decreasing the temperature: decreasing the pressure (by changing the volume): increasing the volume: adding NH4Cl: adding HCl: