The equilibrium constant for the reaction, I2(s) + Br2(g) ⇋ 2 IBr(g) is 0.164 at 25 °C. (a) Calculate ΔrG⦵ for this reaction. (b) Bromine gas is introduced into a container with excess solid iodine. The pressure and temperature are held at 0.164 atm and 25 °C, respectively. Find the partial pressure of IBr(g) at equilibrium. Assume that all the bromine is in the gaseous form and that the vapour pressure of iodine is negligible. (c) In fact, solid iodine has a measurable vapour pressure at 25 °C. In this case, how would the calculation have to be modified?
The equilibrium constant for the reaction, I2(s) + Br2(g) ⇋ 2 IBr(g) is 0.164 at 25 °C. (a) Calculate ΔrG⦵ for this reaction. (b) Bromine gas is introduced into a container with excess solid iodine. The pressure and temperature are held at 0.164 atm and 25 °C, respectively. Find the partial pressure of IBr(g) at equilibrium. Assume that all the bromine is in the gaseous form and that the vapour pressure of iodine is negligible. (c) In fact, solid iodine has a measurable vapour pressure at 25 °C. In this case, how would the calculation have to be modified?
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 60QRT
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The equilibrium constant for the reaction, I2(s) + Br2(g) ⇋ 2 IBr(g) is 0.164 at 25 °C. (a) Calculate ΔrG⦵ for this reaction. (b) Bromine gas is introduced into a container with excess solid iodine. The pressure and temperature are held at 0.164 atm and 25 °C, respectively. Find the partial pressure of IBr(g) at equilibrium. Assume that all the bromine is in the gaseous form and that the vapour pressure of iodine is negligible. (c) In fact, solid iodine has a measurable vapour pressure at 25 °C. In this case, how would the calculation have to be modified?
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