Question

one mole of Ethanol is completely burnt with a produced 1367 kilojoule perm write the chemical equation for this process​

Answer 1

Explanation:

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Answer 2

Answer:

Theoretically about 0.7 g.

Explanation:

First, work out how much energy is involved in heating the water.

E=m.c.θ

E is the energy in J, m is the mass in kg, c is the specific heat of water which is 4186 J/kg.°C and

θ

is the temperature increase. It is fine to assume density of water as 1 g.cm−3

E = 0.2 x 4186 x 24 = 20,092.8 J (or 20.0928 kJ)

1 mole of ethanol when combusted releases 1367 kJ of energy. So to obtain 20.0928 kJ you need (20.0928/1367) = 0.0147 moles.

Molar mass of ethanol is 46.07 g/mol, so you need 0.0147 x 46.07 = 0.68 g of ethanol.

However, this is a theoretical quantity only, as in practise heat energy will be lost to the environment and apparatus during the combustion.

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