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The reaction of bromine gas with chlorine gas, shown here, has a K, value of 7.20 at 200°C. If a closed vessel was charged with the two reactants, each at an initial concentration of 0.200 M, but with no initial concentration of BrC1, what would be the equilibrium concentration of BrCl(g)? Br₂(g) + Cl₂(g) 2BrCl(g) K=7.20

The reaction of bromine gas with chlorine gas, shown here, has a K, value of 7.20 at 200°C. If a closed vessel was charged with the two reactants, each at an initial concentration of 0.200 M, but with no initial concentration of BrC1, what would be the equilibrium concentration of BrCl(g)? Br₂(g) + Cl₂(g) 2BrCl(g) K=7.20

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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Please help me solve the reactions using extent reaction method and ICE method (both answers would be equal at the end). I will give an absolute thumbs up. Step by step please. 

 

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The reaction of bromine gas with chlorine gas, shown here, has a K, value of 7.20 at 200°C. If a closed vessel was charged with the two reactants, each at an initial concentration of 0.200 M, but with no initial concentration of BrCl, what would be the equilibrium concentration of BrCl(g)? Br₂(g) + Cl₂(g) 2BrCl(g) K=7.20
Transcribed Image Text:The reaction of bromine gas with chlorine gas, shown here, has a K, value of 7.20 at 200°C. If a closed vessel was charged with the two reactants, each at an initial concentration of 0.200 M, but with no initial concentration of BrCl, what would be the equilibrium concentration of BrCl(g)? Br₂(g) + Cl₂(g) 2BrCl(g) K=7.20
At a particular temperature, 12.0 moles of SO3 is placed into a 3.0-L rigid container, and the SO3 dissociates by the reaction 2SO3(g)2SO₂(g) + O₂(g) At equilibrium, 3.0 moles of SO₂ is present. Calculate K for this reaction.
Transcribed Image Text:At a particular temperature, 12.0 moles of SO3 is placed into a 3.0-L rigid container, and the SO3 dissociates by the reaction 2SO3(g)2SO₂(g) + O₂(g) At equilibrium, 3.0 moles of SO₂ is present. Calculate K for this reaction.
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