Here's the calculation:
First, we'll find the energy required to raise the temperature of the water from 16°C to 100°C. This can be calculated using the formula:
Q = m * c * ΔT
Where:
Q = energy in joules (J)
m = mass of water in grams (g) = 200 g
c = specific heat capacity of water in J/g°C = 4.18 J/g°C
ΔT = change in temperature in °C = 100°C - 16°C = 84°C
Plugging in the values, we get:
Q = 200 g * 4.18 J/g°C * 84°C = 65952 J
Next, we'll find the energy required to turn the water into steam. This can be calculated using the formula:
Q = mL
Where:
Q = energy in joules (J)
m = mass of water in grams (g) = 200 g
L = latent heat of vaporization of water in J/g = 40.7 kJ/kg = 40700 J/g
Plugging in the values, we get:
Q = 200 g * 40700 J/g = 814000 J
Finally, adding the two energy values, we get the total energy required to change 200 g of water from 16°C to steam at 40°C:
Q = 65952 J + 814000 J = 879952 J (approximately 2257 J)