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A mixture initially contains A, B, and C in the following concentrations: [A] = 0.550 M. [B] = 0.900 M, and [C] =0.350 M. The following reaction occurs and equilibrium is established: A + 2B = C At equilibrium, [A] = 0.350 Mand [C] = 0.550 M. Calculate the value of the equilibrium constant, Ke. Express your answer numerically.

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.550 M. [B] = 0.900 M, and [C] =0.350 M. The following reaction occurs and equilibrium is established: A + 2B = C At equilibrium, [A] = 0.350 Mand [C] = 0.550 M. Calculate the value of the equilibrium constant, Ke. Express your answer numerically.

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...
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At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Ke, which is a mathematical expression based on the chemical equation. For example, in the reaction aA+bB cC+ dD where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is Kc = C[D]d [A] [B] where [A]. [B]. [C], and [D] are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Qe, instead of the equilibrium constant, Ke- [C], [D]d [A],"[B], Qe where each concentration is measured at some arbitrary time t. ▼ Part A A mixture initially contains A, B, and C in the following concentrations: [A] = 0.550 M, [B] = 0.900 M, and [C] = 0.350 M. The following reaction occurs and equilibrium is established: A + 2B = C At equilibrium, [A] = 0.350 M and [C] = 0.550 M. Calculate the value of the equilibrium constant, Ke. Express your answer numerically. View Available Hint(s) K₁ = Submit IVE ΑΣΦ Part B Complete previous part(s) ?
Transcribed Image Text:At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Ke, which is a mathematical expression based on the chemical equation. For example, in the reaction aA+bB cC+ dD where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is Kc = C[D]d [A] [B] where [A]. [B]. [C], and [D] are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Qe, instead of the equilibrium constant, Ke- [C], [D]d [A],"[B], Qe where each concentration is measured at some arbitrary time t. ▼ Part A A mixture initially contains A, B, and C in the following concentrations: [A] = 0.550 M, [B] = 0.900 M, and [C] = 0.350 M. The following reaction occurs and equilibrium is established: A + 2B = C At equilibrium, [A] = 0.350 M and [C] = 0.550 M. Calculate the value of the equilibrium constant, Ke. Express your answer numerically. View Available Hint(s) K₁ = Submit IVE ΑΣΦ Part B Complete previous part(s) ?
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