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Genrish500 [490]
3 years ago
6

Estimate the standard internal energy of formation of liquid methyl acetate (methyl ethanoate, ch3cooch3) at 298 k from its stan

dard enthalpy of formation, which is –442 kj mol-1.
Chemistry
2 answers:
LenKa [72]3 years ago
6 0

solution:

the reaction for formation of methyl acetate is\\CH_{3}OH+CH_{3}COOH----------->CH_{3}COOCH_{3}+H_{2}O\\standard internal energy \\\delta u=\delta H -\delta(pv)=\delta H -\delta n\times RT\\where \delta n=change in number of moles=0\\\delta u=\delta H\\=-442kj/mol

aliina [53]3 years ago
5 0

Answer : The standard internal energy of formation of liquid methyl acetate is, -432.1 kJ/mol

Explanation :

The balanced reaction of formation of liquid methyl acetate will be:

3C(s)+3H_2(g)+O_2(g)\rightarrow CH_3COOCH_3(l)

Formula used :

\Delta H=\Delta U+\Delta n_gRT

or,

\Delta U=\Delta H-\Delta n_gRT

where,

\Delta H = change in enthalpy = -442kJ/mol=-442000J/mol

\Delta U = change in internal energy = ?

\Delta n_g = change in moles = 0 - 4 = -4  (from the reaction)

R = gas constant = 8.314 J/mol.K

T = temperature = 298 K

Now put all the given values in the above formula, we get:

\Delta U=\Delta H-\Delta n_gRT

\Delta U=(-442000J/mol)-[(-4mol)\times 8.314J/mol.K\times 298K

\Delta U=-432089.712J/mol=-432.1kJ/mol

Therefore, the standard internal energy of formation of liquid methyl acetate is, -432.1 kJ/mol

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