A weighed quantity of PCI5(s) is sealed in a 100.0-cm³ glass bulb to which a pressure gauge is attached. The bulb is heated to 250°C, and the gauge shows that the pressure in the bulb rises to 0.895 atm. At this temperature, the solid PCI, is all vaporized and also partially dissociated into Cl2(g) and PCI3(g) according to the equation PCI5(g) 2 PCI3(g) + Cl(g) At 250°C, K = 2.15 for this reaction. Assume that the contents of the bulb are at equilibrium and calculate the partial pressure of the three different chemical species in the vessel.

A weighed quantity of PCI5(s) is sealed in a 100.0-cm³ glass bulb to which a pressure gauge is attached. The bulb is heated to 250°C, and the gauge shows that the pressure in the bulb rises to 0.895 atm. At this temperature, the solid PCI, is all vaporized and also partially dissociated into Cl2(g) and PCI3(g) according to the equation PCI5(g) 2 PCI3(g) + Cl(g) At 250°C, K = 2.15 for this reaction. Assume that the contents of the bulb are at equilibrium and calculate the partial pressure of the three different chemical species in the vessel.

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

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 200. mL flask with 4.3 atm of carbon monoxide gas and 4.1 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.5 atm of carbon monoxide gas, 1.3 atm of water vapor and 2.8 atm of carbon dioxide. The engineer then adds another 1.1 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 O
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 500. mL flask with 4.0 atm of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 1.6 atm of nitrogen dioxide gas. The engineer then adds another 2.0 atm of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the pressure of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 5
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 2.0 L flask with 3.2 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.96 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K¸ = ] x10
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 5.0 L flask with 1.3 atm of nitrogen dioxide gas. When the mixture has come to equilibrium she determines that it contains 0.59 atm of nitrogen dioxide gas. The engineer then adds another 0.65 atm of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the pressure of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. Answer Submitted: atm A 13
3.50 mol NOCl was placed in a 3.50 L reaction vessel at 400ºC. After equilibrium was established, it was found that 36% of the NOCl had dissociated according to the equation 2NOCl(g) 2NO(g) + Cl2(g). Calculate the equilibrium constant, Kc, for the reaction. *equilibrium sign in between NOCl and NO
At 165°C, solid bismuth chloride reacts with 0.0417 mol of steam to form the solid bismuth oxychloride and HCl gas. Steam and HCl have a 1:2 stoichiometric ratio in the reactionBiCl3 (s) + H2O (g) BiOCl (s) + 2 HCl (g) When the reaction reaches equilibrium, the gases are transferred without loss to a 2.50-L vessel. The temperature is kept at 165°C. Sufficient silver(I) ion is added to precipitate the chloride as AgCl. 7.29 g of AgCl are obtained. Determine the value of K for the reaction of the chloride with steam at 165°C?
FO Ammonia will decompose into nitrogen and hydrogen at high temperature. An Industrial chemist studying this reaction fills a 500. mL flask with 0.97 atm of ammonia gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.15 atm. Calculate the pressure equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. do Ar K_ =|| x10
h hydrogen sulfide (H₂S) is usually extracted from 'sour' natural gas, it can also be produced directly from gaseous hydrogen and sulfur at high temperatures: File Preview 2H₂(g) + S₂(g) → 2H₂S(g) In one experiment, 1.20 atm of H₂ and 0.720 atm of S₂ were put in an evacuated cylinder. At equilibrium, the total pressure of the system was 1.47 atm. What is equilibrium constant, Kp, for the reaction?
what is the correct answer in this question
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science presented by Macmillan Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. = 1.80 at 250 °C A 0.2584 mol sample of PCI, (g) is injected into an empty 3.65 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCI5] = || 0.005 Incorrect [PCI,] = 0.066 Incorrect
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 75 L tank with 31. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 12. mol of nitrogen dioxide gas. The engineer then adds another 10. mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol x10 Х G
2