Final answer:
To find the heat required to turn 422 g of water at 23.5 °C into 150 °C steam, calculate the heat to increase temperature to 100 °C, then add the heat needed for vaporization.
Step-by-step explanation:
To calculate the amount of heat required to convert 422 g of liquid H₂O at 23.5 °C into steam at 150 °C, we need to take into account two processes: heating the water from 23.5 °C to 100 °C and vaporizing it at 100 °C. We'll use the specific heat of water and the heat of vaporization.
First, determine the heat required to raise the temperature from 23.5 °C to 100 °C using the formula:
q = m × Cs × ΔT
where q is the heat in Joules, m is the mass in grams, Cs is the specific heat capacity (4.184 J/g°C for water), and ΔT is the change in temperature.
For the first step:
q1 = (422 g) × (4.184 J/g°C) × (100°C - 23.5°C)
Then, calculate the heat required to vaporize the water at 100 °C using the heat of vaporization:
q2 = m × ΔHvap
where ΔHvap is the heat of vaporization (2260 J/g for water).
For the second step:
q2 = (422 g) × (2260 J/g)
Combine both amounts of heat:
total heat (qtotal) = q1 + q2
Calculate the totals for q1 and q2, and then sum them to find the total heat required.