Question

How much energy in kJ is released when 15.3 grams of steam at 115.0 degrees Celsius is condensed to give liquid water at 75.0 degrees Celsius? The heat of vaporization of liquid water is 40.67 kJ/mol and the molar heat capacity is 75.4 J/(K x mol) for the liquid and 33.6 J/(K x mol) for the vapor.

Answer 1

The energy released when 15.3 grams of steam condenses to liquid water is approximately 34.57 kJ. Energy released during condensation = 0.8492 mol x 40.67 kJ/mol = 34.57 kJ

Step-by-step explanation:

To calculate the energy released when steam condenses to liquid water, we need to determine the amount of heat absorbed during vaporization and the amount of heat released during condensation.

The heat of vaporization of water is 40.67 kJ/mol.

We can use this information to find the energy released when 15.3 grams of steam condenses to liquid water.

First, we need to calculate the number of moles of steam present.

To do this, we can use the molar mass of water (18.015 g/mol) and the given mass of steam (15.3 grams).

1. Calculate the number of moles of steam:

moles of steam = mass of steam / molar mass of water = 15.3 g / 18.015 g/mol

= 0.8492 mol

Now, we can calculate the energy released during condensation:

Energy released during condensation = moles of steam x heat of vaporization

Energy released during condensation = 0.8492 mol x 40.67 kJ/mol

= 34.57 kJ