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Consider the following equilibrium: H2(g) +12(g) 2 HI(g) At 698 K, the Kp for this reaction is 54.4. If 0.50 mol of H2(g) and 0.10 mol of 12(g) are mixed in a 5.00 L flask at 698 K, what will be the equilibrium concentration of HI(g)?

Consider the following equilibrium: H2(g) +12(g) 2 HI(g) At 698 K, the Kp for this reaction is 54.4. If 0.50 mol of H2(g) and 0.10 mol of 12(g) are mixed in a 5.00 L flask at 698 K, what will be the equilibrium concentration of HI(g)?

Chemistry & Chemical Reactivity
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 equilibrium: H2(g) +12(g) 2 HI(g) At 698 K, the Kp for this reaction is 54.4. If 0.50 mol of H2(g) and 0.10 mol of 12(g) are mixed in a 5.00 L flask at 698 K, what will be the equilibrium concentration of HI(g)?
Transcribed Image Text:Consider the following equilibrium: H2(g) +12(g) 2 HI(g) At 698 K, the Kp for this reaction is 54.4. If 0.50 mol of H2(g) and 0.10 mol of 12(g) are mixed in a 5.00 L flask at 698 K, what will be the equilibrium concentration of HI(g)?
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