Chemistry Class 11 NCERT Solutions: Chapter 7 Equilibrium Part 6

Chemistry Class 11 NCERT Solutions Chapter 7 Equilibrium Part 6

Q: 17. Equation at Equation for the equilibrium shown below. What is the equilibrium concentration of Equation when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

Equation

Answer:

Let p be the pressure exerted by ethane and hydrogen gas (each) at equilibrium. Now, according to the reaction,

Equation

Equation

Equation

Equation

Equation

Now, p Equation

Equation

Equation (Taking positive value)

Equation

Hence, at equilibrium,

Equation

Equation

Q: 18. Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as:

Equation

Structure of Acetic Acid

Structure of Acetic Acid

Structure of Acetic Acid

(i) Write the concentration ratio (reaction quotient), Qc, this reaction (note: water is not in excess and is not a solvent in this reaction)

(ii) At 293 K, if one starts with 1.00 mol of acetic acid and 0.18 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant

(iii) Starting with 0.5 of ethanol and 1.0 mol of acetic acid and maintaining it at 293 K, 0.214 mol of ethyl acetate is found after sometime. Has equilibrium been reached?

(i) Reaction quotient, Equation

(ii) Let the volume of the reaction mixture be V. Also, here we will consider that water is a solvent and present in excess.

The given reaction is:

Equation

Therefore, equilibrium constant for the given reaction is:

Equation

Equation

Equation

(iii) Let the volume of the reaction mixture be V.

Equation

Therefore, the reaction quotient is,

Equation

Equation

Equation

Equation

Since Equation equilibrium has not been reached.

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