Pure butanol is to be fed into a semibatch reactor containing pure ethyl acetate to produce butyl acetate and ethanol. The react
ion
CH_3COOC_2H_5 + C_4H_9OH <--------> CH_3COOC_4H_9 + C_2H_5OH
is elementary and reversible. The reaction is carried out isothermally at 300 K. At this the equilibrium constant is 1.08 and the specific reaction rate is 9 x 10^-5 dm^3/mol*s. Initially, there is 200 dm^3 of ethyl acetate in the vat, and butanol is fed at a volumetric rate of 0.05 dm^3/ s. The feed and initial concentrations of butanol and ethyl acetate are 10.93 mol/dm^3 and .72 molu/dm^3, respectively.
(a) Plot and analyze the equilibrium conversion of ethyl acetate as a function of time.
(b) Plot and analyze the conversion of ethyl acetate, the rate of reaction, and the concentration of butanol as a function of time.
CH_3COOC_2H_5 + C_4H_9OH <--------> CH_3COOC_4H_9 + C_2H_5OH
is elementary and reversible. The reaction is carried out isothermally at 300 K. At this the equilibrium constant is 1.08 and the specific reaction rate is 9 x 10^-5 dm^3/mol*s. Initially, there is 200 dm^3 of ethyl acetate in the vat, and butanol is fed at a volumetric rate of 0.05 dm^3/ s. The feed and initial concentrations of butanol and ethyl acetate are 10.93 mol/dm^3 and .72 molu/dm^3, respectively.
(a) Plot and analyze the equilibrium conversion of ethyl acetate as a function of time.
(b) Plot and analyze the conversion of ethyl acetate, the rate of reaction, and the concentration of butanol as a function of time.
1 answer:
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Answer:
The force between the charges when the separation decreases to 0.7 meters equals 126.955 Newtons
Explanation:
We know that for two point charges of magnitude the magnitude of force between them is given by
where
is constant
is the separation between the charges
Initially when the charges are separated by 2.4 meters the force can be calculated as
Now when the separation is reduced to 0.7 meters the force is similarly calculated as
Applying value of the constant we get
Thus
Answer:
Explanation:
Hello,
In this case by combining the first and second law of thermodynamics for this ideal gas, we can obtain the following expression for the differential of the specific entropy <em>at constant pressure</em>:
Whereas Rg is the specific ideal gas constant for the studied gas; thus, integrating:
We obtain the expression to compute the specific entropy change:
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