III Calculations Involving the Equilibrium Constant A. One mole of acetic acid, CH3COOH, and 1 mole of ethanol, C2H5OH, were reacted in one- liter vessel and allowed to attain equilibrium at 25°C. The equilibrium mixture was then titrated with standard base and was found to contain 0.667 moles of acetic acid after the following reaction has taken place to form ethyl acetate and water. Supply the table and calculate the equilibrium constant (Kc) CH3COOH(soln) + C2H5OH(soln) C2H5OOCCH(soln). H2O 0 Initial Concentration 1.000 M 1.000 M Change in Concentration Equilibrium Concentration B. For the reaction, 3H2 H2, 0.10 mole N2, and 0.20 mole NH3 are placed in an empty 1.0-liter vessel at 1000K, toward which direction will the reaction proceed? -0.667 M 0.333 М + N2g) + 2NH3 (g), Ke = 2.4 x 10-3 at 1000K. If 0.30 mole (g)
III Calculations Involving the Equilibrium Constant A. One mole of acetic acid, CH3COOH, and 1 mole of ethanol, C2H5OH, were reacted in one- liter vessel and allowed to attain equilibrium at 25°C. The equilibrium mixture was then titrated with standard base and was found to contain 0.667 moles of acetic acid after the following reaction has taken place to form ethyl acetate and water. Supply the table and calculate the equilibrium constant (Kc) CH3COOH(soln) + C2H5OH(soln) C2H5OOCCH(soln). H2O 0 Initial Concentration 1.000 M 1.000 M Change in Concentration Equilibrium Concentration B. For the reaction, 3H2 H2, 0.10 mole N2, and 0.20 mole NH3 are placed in an empty 1.0-liter vessel at 1000K, toward which direction will the reaction proceed? -0.667 M 0.333 М + N2g) + 2NH3 (g), Ke = 2.4 x 10-3 at 1000K. If 0.30 mole (g)
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:III Calculations Involving the Equilibrium Constant
A. One mole of acetic acid, CH3COOH, and 1 mole of ethanol, C2H5OH, were reacted in one-
liter vessel and allowed to attain equilibrium at 25°C. The equilibrium mixture was then
titrated with standard base and was found to contain 0.667 moles of acetic acid after
the following reaction has taken place to form ethyl acetate and water. Supply the table
and calculate the equilibrium constant (Kc)
CH3COOH(soln) +
C2H5OH(soln)
C2H5OOCCHsoln).
H2O (1)
Initial
1.000 M
1.000 М
Concentration
Change in
Concentration
-0.667 M
Equilibrium
Concentration
0.333 M
+ 2NH3 (g), Ke = 2.4 x 10-3 at 1000K. If 0.30 mole
B. For the reaction, 3H2 (g) + N2(g)
H2, 0.10 mole N2, and 0.20 mole NH3 are placed in an empty 1.0-liter vessel at 1000K,
toward which direction will the reaction proceed?
%3D
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