# Chemistry Class 11 NCERT Solutions Chapter 7 Equilibrium Part 6

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

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

Now, p

(Taking positive value)

Hence, at equilibrium,

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

(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,

(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:

Therefore, equilibrium constant for the given reaction is:

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

Therefore, the reaction quotient is,

Since equilibrium has not been reached.

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