Acetic acid and ethanol react to form ethyl acetate and water, like this: HCH, CO2(aq) + C2H5OH(aq) right arrow C2H, CO2CH3(aq) + H2O
Imagine 246. mmol of C2HCO2CH3 Imagineofare removed from a flask containing a mixture of, andat equilibrium,
1. What is the rate of the reverse reaction before any C2HsCO2CH3 has been removed from the flask?
A. Zero.
B. Greater than zero, but less than the rate of the forward reaction.
C. Greater than zero, and equal to the rate of the forward reaction.
D. Greater than zero, and greater than the rate of the forward reaction.
2. What is the rate of the reverse reaction just after the CoHsCO CH has been removed from the flask?
A. Zero.
B. Greater than zero, but less than the rate of the forward reaction.
C. Greater than zero, and equal to the rate of the forward reaction.
D. Greater than zero, and greater than the rate of the forward reaction.
3. What is the rate of the reverse reaction when the system has again reached equilibrium?
A. Zero.
B. Greater than zero, but less than the rate of the forward reaction.
C. Greater than zero, and equal to the rate of the forward reaction.
D. Greater than zero, and greater than the rate of the forward reaction.
4. How much less C2H5CO2CH3 is in the flask when the system has again reached equilibrium?
A. Zero.
B. Greater than zero, but less than the rate of the forward reaction.
C. Greater than zero, and equal to the rate of the forward reaction.
D. Greater than zero, and greater than the rate of the forward reaction.

1.) Option C is correct.

The rate of reverse reaction is greater than zero, but equal to the rate of the forward reaction.

2) Option B is correct.

The rate of reverse reaction is Greater than zero, but less than the rate of the forward reaction.

3) Option C is correct.

The rate of reverse reaction is Greater than zero, and equal to the rate of the forward reaction.

4) Option A is correct.

How much less C2H5CO2CH3 is in the flask when the system has again reached equilibrium? Zero.

Explanation:

HCH,CO2(aq) + C2H5OH(aq) ⇌ C2H,CO2CH3(aq) + H2O

1) Before the main product is removed from the reaction setup, the chemical reaction is at equilibrium.

Chemical equilibrium is a state of dynamic equilibrium such that the concentration of the reactants and the products do not always remain the same but the rate of forward reaction always matches the rate of backward reaction.

2) When 246. mmol of C2HCO2CH3 are removed from the reaction mixture

And when one of the factors involved in chemical equilibrium changes, Le Chatellier's principle explains that the system then adjusts to remedy this change and takes time to go back to equilibrium again.

When one of the species involved in the chemical reaction at equilibrium, is removed from the reaction mixture, the rate of reaction begins to favour that side of the reaction until equilibrium is re-established.

So, when 246 mmol of one of the products is removed, the response is to cause the rate of forward reaction to be favoured to produce more of products as there are fewer, and the rate of reverse reaction at this moment becomes less than the rate of forward reaction.

3) The rate of the reverse reaction when the system has again reached equilibrium

Like I said in (2) above, the reaction remedies this change in concentration of one of the products until equilibrium is re-established and when chemical equilibrium is re-established the rate of forward reaction once again matches the rate of backward reaction.

4) How much less C2H5CO2CH3 is in the flask when the system has again reached equilibrium?

By the time equilibrium is re-established, the system goes back to how it all was and the concentration of C2H5CO2CH3 goes back to the same as it was at the start of the reaction.

Hope this Helps!!!

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