Acetic acid (CH3COOH) dissociates in waterand exists in equilibrium with its ionsaccording to the following chemicalequation:СНЗСООН аg-CHЗСОO-аq+H+аqThe value of the equilibrium constant at25°C is 1.8*10-5. What does this value tell you about therelative amount of reactant and products atequilibrium?

We have to predict the relative amount of product and Reactant at equilibrium

Acetic acid (CH3COOH) dissociates in water and exists in equilibrium with its ions according to the following chemical equation: СНЗСООН аq %3D СНЗСОО-аq+H+аq The value of the equilibrium constant at 25°C is 1.8*10-5 What does this value tell you about the relative amount of reactant and products at equilibrium?

Acetic acid (CH3COOH) dissociates in water and exists in equilibrium with its ions according to the following chemical equation: СНЗСООН аq %3D СНЗСОО-аq+H+аq The value of the equilibrium constant at 25°C is 1.8*10-5 What does this value tell you about the relative amount of reactant and products at equilibrium?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 53QRT: Consider the equilibrium N2(g)+O2(g)2NO(g) At 2300 K the equilibrium constant Kc = 1.7 103. If 0.15...

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Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
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Consider the equilibrium N2(g)+O2(g)2NO(g) At 2300 K the equilibrium constant Kc = 1.7 103. If 0.15 mol NO(g) is placed into an empty, sealed 10.0-L flask and heated to 2300 K, calculate the equilibrium concentrations of all three substances at this temperature.
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?