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Chapter 13: Q30E (page 752)

What is the approximate value of the equilibrium constant KP for the change C2H5OC2H5 (l)⇌C2 H5OC2H5 (g) at 25 °C.

(Vapor pressure was described in the previous chapter on liquids and solids; refer back to this chapter to find the relevant information needed to solve this problem.)

Short Answer

Expert verified

\({K_p} = 0.7\;{\rm{atm}}{\rm{.}}\)

Step by step solution

01

Vapor pressure of Diethyl ether:

The reaction given

The pressure of a diethyl ether vapor at 25oc is \(0.7\;{\rm{atm}}{\rm{.}}\)

02

The approximate value of the equilibrium constant KP:

Let us calculate the equilibrium constant \({{\rm{K}}_{\rm{p}}}\) for the change at 25oc

The equilibrium constant\({{\rm{K}}_{\rm{p}}}:\)

\(\begin{array}{l}{K_p} = \frac{{{P_{{C_2}{H_5}O{C_2}{H_5}(g)}}}}{1}\\\;\;\;\;\; = {P_{{C_2}{H_5}O{C_2}{H_5}(g)}}\\\;\;\;\;\; = 0.7\;{\rm{atm}}{\rm{.}}\end{array}\)

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Most popular questions from this chapter

Write the expression of the reaction quotient for the ionization of HOCN in water.

Determine if the following system is at equilibrium. If not, in which direction will the system need to shift to reach equilibrium?

\({\rm{S}}{{\rm{O}}_2}{\rm{C}}{{\rm{l}}_2}(g)\rightleftharpoons {\rm{S}}{{\rm{O}}_2}(g) + {\rm{C}}{{\rm{l}}_2}(g)\)

\(\left( {{\rm{S}}{{\rm{O}}_2}{\rm{C}}{{\rm{l}}_2}} \right) = 0.12\;{\rm{M}},\;\left( {{\rm{C}}{{\rm{l}}_2}} \right) = 0.16\;{\rm{M and }}\left( {{\rm{S}}{{\rm{O}}_2}} \right) = 0.050\;{\rm{M}}.\;{K_c}\) for the reaction is 0.078.

Question: Calculate the equilibrium concentrations that result when 0.25 M O2 and 1.0 M HCl react and come to equilibrium.

Question: The density of trifluoroacetic acid vapor was determined at 118.1 °C and 468.5 torr, and found to be 2.784 g/L.

CalculateKcfor the association of the acid.

Question : A 0.010Msolution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 °C. A 0.010Msolution of the weak acid HB has an osmotic pressure of 0.345 atm under the same conditions.

(a) Which acid has the larger equilibrium constant for ionization

HA[HA(aq) ⇌ A−(aq) + H+(aq)]or HB[HB(aq) ⇌ H+(aq) + B−(aq)]?

(b) What are the equilibrium constants for the ionization of these acids?

(Hint: Remember that each solution contains three dissolved species: the weak acid (HA or HB), the conjugate base (A− or B−), and the hydrogen ion (H+). Remember that osmotic pressure (like all colligative properties) is related to the total number of solute particles. Specifically for osmotic pressure, those concentrations are described by molarities.)
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