Acetic acid and ethanol react to form ethyl acetate and water, like this: HCH_3
ID: 1004968 • Letter: A
Question
Acetic acid and ethanol react to form ethyl acetate and water, like this: HCH_3 CO_2(aq) + C_2 H_5 OH(aq) rightarrow C_2 H_5 CO_2 CH_3 (aq) + H_2 O(I) Imagine 182. mmol of HCH_3 CO_2 are removed from a flask containing a mixture of HCH_3 CO_2, C_2 H_5 OH, C_2 H_5 CO_2 CH_3 and H_2 O at equilibrium, and then answer the following questions. What is the rate of the forward reaction before any HCH_3 CO_2 has been removed from the flask? Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. What is the rate of the forward reaction just after the HCH_3 CO_2 has been removed from the flask? Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. What is the rate of the forward reaction when the system has again reached equilibrium? Zero. Greater than zero, but less than the rate of the reverse reaction. Greater than zero, and equal to the rate of the reverse react on. Greater than zero, and greater than the rate of the reverse reaction. How much less HCH_3 CO_2 is in the flask when the system has again reached equilibrium? None. Some, but less than 182. mmol. 182. mmo!. More than 182. mmol.Explanation / Answer
Answer – We are given the reaction between acetic acid and ethanol to from ethyl acetate and water.
Reaction –
HCH3CO2(aq) + C2H5OH(aq) -----> C2H5CO2(aq) + H2O(l)
According to the Le Chatelier's principle, when we remove the concentration of one side then the equilibrium shifted towards the same side.
The rate of the forward reaction before any HCH3CO2 has been removed from the flask is Greater than zero, and equal to the rate of the reverse reaction, because we know at equilibrium the rate of forward reaction is equal to the rate of reverse reaction.
The rate of the forward reaction just after the HCH3CO2 has been removed from the flask is Greater than zero, but less than the rate of the reverse reaction, because when we remove the concentration of acetic acid from reactant side then equilibrium will shift towards reactant side, means rate of forward reaction is less than reverse reaction.
When system of the forward reaction has again reached equilibrium then rate of forward reaction is Greater than zero, and equal to the rate of the reverse reaction, because we know at equilibrium the rate of forward reaction is equal to the rate of reverse reaction.
The HCH3CO2 is in the flask when the system has again reached equilibrium is more than 182. mmol, because when the system has again reached equilibrium then there is formed HCH3CO2 means the removed HCH3CO2 is formed again which is more than removed 182. mmol.
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