2. Phosphorous pentachloride is a fine grained powder, ranging in colour from colourless to pale yellow. It has a pungent odour. In the gaseous state it shows the equilibrium shown in the equation below. Initially, a sample of phosphorus pentachloride is introduced to an empty vessel. If the equilibrium constant for the above reaction is 5.7 x 10-4 and the equilibrium concentration of [PCI (g)] is 0.0830 mol/L, the equilibrium concentration of [PC1₂(g)] is mol/L. SHOW ALL YOUR WORK. PC1₂(g) → PCl₂(g) + Cl₂(g)

2. Phosphorous pentachloride is a fine grained powder, ranging in colour from colourless to pale yellow. It has a pungent odour. In the gaseous state it shows the equilibrium shown in the equation below. Initially, a sample of phosphorus pentachloride is introduced to an empty vessel. If the equilibrium constant for the above reaction is 5.7 x 10-4 and the equilibrium concentration of [PCI (g)] is 0.0830 mol/L, the equilibrium concentration of [PC1₂(g)] is mol/L. SHOW ALL YOUR WORK. PC1₂(g) → PCl₂(g) + Cl₂(g)

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 equilibrium constant, K, for the following reaction is 2.31×10-4 at 548 K. NH4Cl(s) NH3(g) + HCl(g) An equilibrium mixture in a 13.3 L container at 548 K contains 0.359 mol NH4Cl(s), 1.90×10-2 M NH3 and 1.22×10-2 M HCl. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 6.29 L? [NH3] = M [HCl] = M
he equilibrium constant, K, for the following reaction is 1.80×10-4 at 298 K.NH4HS (s) NH3 (g) + H2S (g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.219 mol NH4HS, 1.34×10-2 M NH3 and 1.34×10-2 M H2S. If the concentration of H2S(g) is suddenly increased to 2.32×10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished?
The equilibrium constant, K, for the following reaction is 1.80×10-4 at 298 K. NH3(g) + H₂S(g) NH4HS(s) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.366 mol NH4HS, 1.34×10- M NH3 and 1.34×10-² M H₂S. If the concentration of NH3(g) is suddenly increased to 2.41x10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [H₂S] = ΣΣ M
Which is the correct equilibrium constant expression for the following reactiont OK Fez Os(s) + 3H2(g) +2 Fe(s) + 3H2O(g) = [Fe2O3][H2] [Fe][H2O3 OK [Fe][H2O3 = [Fe2O3][H2]3 OK [H2O] = [H2] K OK = [Fe][H2O] [Fe2O3] [H2] [H2O] 3 H23
Calculating an equilibrium constant from a partial equilibrium composition Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 500. mL flask with 3.3 atm of ammonia gas and 0.87 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.6 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 P ☐ x1 x10 ☑ 5
The equilibrium constant, K, for the following reaction is 2.53×10-2 at 519 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 17.8 L container at 519 K contains 0.233 M PCl5, 7.68×10-2 M PCl3 and 7.68×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 8.95 L? [PCl5] = M [PCl3] = M [Cl2] = M
A chemical engineer is studying the following reaction: HCH3CO2(aq)+CH3NH2(aq) → CH3CO2(aq) + CH3NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.54. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound concentration expected change in concentration HCH,CO₂ 1.01 M O↑ increase CH3NH2 1.22 M O decrease O↑ increase O decrease O (no change) O (no change) A CH,CO, 0.64 M O↑ increase O decrease O (no change) CH, NH3 1.04 M O ↑ increase O decrease O (no change) HCH CO₂ 0.33 M O↑ increase O decrease O(no change) CHÍNH, 0.50 M O↑ increase O decrease O (no change) B CH,CO, 1.01 M O increase O decrease O (no…
A student ran the following reaction in the laboratory at 543 K: CoCl₂(g) CO(g) + Cl₂(g) When she introduced 1.10 moles of COCI₂(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.94-102 M. Calculate the equilibrium constant, K, she obtained for this reaction.