Br₂(g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 198.0 L flask initially contains 1.047 kg of Br₂ and 1.169 kg of Cl₂. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: What is the percent yield of BrCl? g
Br₂(g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 198.0 L flask initially contains 1.047 kg of Br₂ and 1.169 kg of Cl₂. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: What is the percent yield of BrCl? g
General Chemistry - Standalone book (MindTap Course List)
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Chapter14: Chemical Equilibirum
Section: Chapter Questions
Problem 14.19QP: During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction...
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The expression of equilibrium constant (in terms of partial pressure) in any reaction is
Kc = equilibrium constant in terms of concentration
R = universal gas constant
= moles of products - moles of reactants
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