Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2 IBr(g) Kc = 1.1 × 10^2 @ 25 o C A reaction mixture initially contains 0.50 moles of Br2 and I2 in a 3.0 L vessel. Calculate the equilibrium concentration of I2, Br2 and IBr. Using the data from above, calculate Kc for the following reaction: 4 IBr(g). ⇌ 2I2(g) + 2Br2(g)
Consider the following reaction and its equilibrium constant: I2(g) + Br2(g) ⇌ 2 IBr(g) Kc = 1.1 × 10^2 @ 25 o C A reaction mixture initially contains 0.50 moles of Br2 and I2 in a 3.0 L vessel. Calculate the equilibrium concentration of I2, Br2 and IBr. Using the data from above, calculate Kc for the following reaction: 4 IBr(g). ⇌ 2I2(g) + 2Br2(g)
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.4: Using Equilibrium Constants In Calculations
Problem 15.5CYU: The decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the...
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Consider the following reaction and its equilibrium constant:
I2(g) + Br2(g) ⇌ 2 IBr(g) Kc = 1.1 × 10^2 @ 25 o C
A reaction mixture initially contains 0.50 moles of Br2 and I2 in a 3.0 L vessel. Calculate the
equilibrium concentration of I2, Br2 and IBr.
Using the data from above, calculate Kc for the following reaction:
4 IBr(g). ⇌ 2I2(g) + 2Br2(g)
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