Final answer:
Calculating the total heat required to convert 431 g of liquid water at 23.4°C into steam at 144°C involves three steps: heating the water to the boiling point,
Step-by-step explanation:
The question asks how much heat (in kilojoules) is required to convert 431 g of liquid H₂O at 23.4°C into steam at 144°C. To find the answer, several steps are required: first, heating the liquid water from the initial temperature to the boiling point, then vaporizing the water into steam, and finally, heating the steam
To calculate the heat needed to raise the temperature of liquid water to its boiling point (100°C), we use the formula Q = mcΔT, where m is the mass of the water, c is the specific heat capacity of water (4.184 J/g°C), and ΔT is the change in temperature. To vaporize the water into steam, we use water's heat of vaporization (ΔHvap = 2260 J/g).
Finally, we calculate the heat required to raise the temperature of the steam to the final temperature using the specific heat capacity of steam, which is lower than that of liquid water.
The total heat required is the sum of the heat to raise the temperature of the liquid water to boiling, the heat of vaporization to convert the water to steam, and the heat to raise the temperature of the steam to the final temperature.