Heat energy full question is in description

Question

 How much heat energy is required to convert 88.5 g of solid ethanol at −114.5°C to gasesous ethanol at 167.1 C The molar heat of fusion of ethanol is 4.60 kJ/mol and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of −114.5°C and a normal boiling point of 78.4°C. The specific heat capacity of liquid ethanol is 2.45J/g⋅°C and that of gaseous ethanol is 1.43J/g⋅

Answer 1

To calculate the heat energy required for the given process, we need to consider the different stages involved: melting the solid ethanol, heating the liquid ethanol to its boiling point, and then vaporizing it.

First, let's calculate the heat energy required to melt the solid ethanol. We can use the formula:

Heat energy = mass × molar heat of fusion

For the given mass of 88.5 g, we can convert it to moles using the molar mass of ethanol. The molar mass of ethanol is approximately 46.07 g/mol.

Moles of ethanol = mass / molar mass

Next, we can calculate the heat energy required to melt the solid ethanol:

Heat energy for melting = moles of ethanol × molar heat of fusion

Now, let's calculate the heat energy required to raise the temperature of the liquid ethanol from its melting point to its boiling point. We can use the formula:

Heat energy = mass × specific heat capacity × temperature change

The temperature change is the difference between the boiling point (78.4°C) and the melting point (-114.5°C).

Finally, we can calculate the heat energy required to vaporize the liquid ethanol. We can use the formula:

Heat energy = moles of ethanol × molar heat of vaporization

By summing up the heat energies for each stage, we can determine the total heat energy required.