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ANEK [815]
3 years ago
5

Conversion of 0.702 g of liquid water to steam at 100.0°C requires 1.56 kJ of heat. Calculate the molar enthalpy of evaporation

of water at 100.0°C.
Chemistry
1 answer:
kifflom [539]3 years ago
7 0

Answer:

The molar enthalpy of evaporation of water at 100.0°C is 40 kJ

Explanation:

Calculation of the moles of H_2O as:-

Mass = 0.702 g

Molar mass of H_2O = 18 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{0.702\ g}{18\ g/mol}

Moles= 0.039\ mol

Given that:- \Delta H=+1.56\ kJ

It means that when 0.039 moles of water undergoes evaporation, 1.56 kJ of energy is used

Also,

When 1 mole of water undergoes evaporation, \frac{1.56}{0.039}\ kJ of energy is used

<u>The molar enthalpy of evaporation of water at 100.0°C is 40 kJ</u>

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