The industrial solvent ethyl acetate is produced by the reaction of acetic acid with ethanol: C H 3 C O 2 O H ( s o ln ) + C H 3 C H 2 O H ( s o ln ) ⇌ C H 3 C O 2 C H 2 C H 3 ( s o ln ) + H 2 O ( s o ln ) C H 3 C O 2 H ( s o ln ) + H 3 C H 2 O H ( s o ln ) ⇌ C H 3 C O 2 C H 3 ( S o ln ) + H 2 O ( S o ln ) A c e t i c A c i d E t h a n o l E t h y l a c e t a t e Write the equilibrium constant expression for K c . A solution prepared by mixing 1.00 mol of acetic acid and 1.00 mol of ethanol contains 0.65 moI of ethyl acetate at equilibrium. Calculate the value of K c . Explain why you can calculate K c without knowing the volume of the solution.
The industrial solvent ethyl acetate is produced by the reaction of acetic acid with ethanol: C H 3 C O 2 O H ( s o ln ) + C H 3 C H 2 O H ( s o ln ) ⇌ C H 3 C O 2 C H 2 C H 3 ( s o ln ) + H 2 O ( s o ln ) C H 3 C O 2 H ( s o ln ) + H 3 C H 2 O H ( s o ln ) ⇌ C H 3 C O 2 C H 3 ( S o ln ) + H 2 O ( S o ln ) A c e t i c A c i d E t h a n o l E t h y l a c e t a t e Write the equilibrium constant expression for K c . A solution prepared by mixing 1.00 mol of acetic acid and 1.00 mol of ethanol contains 0.65 moI of ethyl acetate at equilibrium. Calculate the value of K c . Explain why you can calculate K c without knowing the volume of the solution.
Solution Summary: The author explains the equilibrium constant expression for K_ c, which is defined as ratio of concentration of product to reactant raise to the power of their stoichiometric
The industrial solvent ethyl acetate is produced by the reaction of acetic acid with ethanol:
C
H
3
C
O
2
O
H
(
s
o
ln
)
+
C
H
3
C
H
2
O
H
(
s
o
ln
)
⇌
C
H
3
C
O
2
C
H
2
C
H
3
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s
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ln
)
+
H
2
O
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s
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)
C
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C
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+
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C
H
2
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⇌
C
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C
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2
C
H
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+
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2
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S
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)
A
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Write the equilibrium constant expression for
K
c
.
A solution prepared by mixing 1.00 mol of acetic acid and 1.00 mol of ethanol contains 0.65 moI of ethyl acetate at equilibrium. Calculate the value of
K
c
. Explain why you can calculate
K
c
without knowing the volume of the solution.
When baking soda (NaHCO3) is heated at a certain temperature, it releases carbo dioxide gas, which is responsible for the rising of cookies, doughnuts, and bread. The reaction involved is shown below as follows:
2NaHCO3(s) ⇌ Na2CO3(s) + H2O(g) + CO2(g)
What is the Keq of the reaction, given that the concentrations at equilibrium of water and carbon dioxide are 1.15 x 103 M and 2.35 x 103 M respectively?
Calomel, Hg2Cl2, is a compound composed of the diatomic ion of mercury(I), Hg2 2+, and chloride ions, Cl–. Although most mercury compounds are now known to be poisonous, eighteenth-century physicians used calomel as a medication. Their patients rarely suffered any mercury poisoning from the treatments because calomel is quite insoluble:Hg2 Cl2(s) ⇌ Hg2 2+(aq) + 2Cl−(aq) Ksp = 1.1 × 10−18Calculate the molar solubility of Hg2Cl2.
Consider the reaction: HSO4-(aq) + H2O(l) ⇌ H3O+(aq) + SO42-(aq)
Drops of sodium sulfate solution are added to 10 drops of sodium hydrogen sulfate solution until a reaction occurs. The reaction indicated a shift in the point of equilibrium. In which direction did the equilibrium shift?
Crystals of solid sodium hydrogen sulfate are added to 10 drops of sodium hydrogen sulfate solution until a reaction occurs. The reaction indicated a shift in the point of equilibrium. In which direction did the equilibrium shift?
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