The equilibrium constant, Ke, for the following reaction is 5.10 x 10 at 548 K. NH₂Cl(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 4.06 L container at 548 K contains 1.08 mol of NH₂Cl(s) and 0.368 mol of NH3, the number of moles of HCI present is mol, A student ran the following reaction in the laboratory at 696 K: 2HI(g) H₂(g) + 1₂ (9) When she introduced HI(g) at a pressure of 3.15 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of 1₂ (9) to be 0.333 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction.

The equilibrium constant, Ke, for the following reaction is 5.10 x 10 at 548 K. NH₂Cl(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 4.06 L container at 548 K contains 1.08 mol of NH₂Cl(s) and 0.368 mol of NH3, the number of moles of HCI present is mol, A student ran the following reaction in the laboratory at 696 K: 2HI(g) H₂(g) + 1₂ (9) When she introduced HI(g) at a pressure of 3.15 atm into a 1.00 L evacuated container, she found the equilibrium partial pressure of 1₂ (9) to be 0.333 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 62QRT

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