The equilibrium constant, K, for the following reaction is 1.29x10-² at 600K. COCI₂(g)CO(g) + Cl₂(g) If an equilibrium mixture of the three gases in a 15.7 L container at 600K contains 0.288 mol of COCI₂(g) and 0.403 mol of CO, the equilibrium concentration of Cl₂ is M. Submit Answer Retry Entire Group 7 more group attempts remaining The equilibrium constant, Kc, for the following reaction is 1.80x10-4 at 298 K. NH4HS(s) NH3(g) + H₂S(g) If an equilibrium mixture of the three compounds in a 5.15 L container at 298 K contains 1.71 mol of NH4HS(s) and 0.380 mol of NH3, the number of moles of H₂S present is moles. Submit Answer Retry Entire Group 7 more group attempts remaining
The equilibrium constant, K, for the following reaction is 1.29x10-² at 600K. COCI₂(g)CO(g) + Cl₂(g) If an equilibrium mixture of the three gases in a 15.7 L container at 600K contains 0.288 mol of COCI₂(g) and 0.403 mol of CO, the equilibrium concentration of Cl₂ is M. Submit Answer Retry Entire Group 7 more group attempts remaining The equilibrium constant, Kc, for the following reaction is 1.80x10-4 at 298 K. NH4HS(s) NH3(g) + H₂S(g) If an equilibrium mixture of the three compounds in a 5.15 L container at 298 K contains 1.71 mol of NH4HS(s) and 0.380 mol of NH3, the number of moles of H₂S present is moles. Submit Answer Retry Entire Group 7 more group attempts remaining
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.36PAE: The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of...
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