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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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The compound dioxane, which is used as a solvent in various industrial processes is composed of C,H, and O atoms. Combustion of
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Answer:

The correct formula of dioxane is C₄H₈O₂.

Explanation:

Given data:

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mass of water = 1.802 g

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molar mass of dioxane = 88.1 g / mol

Molecular formula of dioxane = ?

Solution:

percentage of carbon = (4.401 g/2.23 g ) × (12 /44) × 100

                                     =  (1.98 × 0.273) × 100 = 54.1

percentage of hydrogen =  (1.802 g/ 2.23 g) × (2.016 /18.016) × 100

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Now we will determine the number of grams atoms of carbon, hydrogen and oxygen.

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No. of gram atoms of hydrogen = 9.072 / 1.008 = 9

No. of gram atoms of oxygen = 36.828 / 16 = 2.302

Atomic ratio:

    C :H :O               4.51/ 2.302    :   9 / 2.302   :  2.302 /2.302

    C :H :O                2 : 4 : 1

Molecular formula:

   Molecular formula = n × (empirical formula)

   n = molar mass of compound / empirical formula mass

   empirical formula mass= 2 × 12 + 4 × 1.008  + 1 × 16

    empirical formula mass= 24+ 4.032 +16 = 44.032

                 n = 88.1 / 44.032 = 2

        Molecular formula = n × (empirical formula)

        Molecular formula = 2 × (C₂H₄O)

         Molecular formula = C₄H₈O₂

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