Final answer:
The correct answer to the amount of energy transferred to water as heat when a hot copper cylinder is dropped into it, causing some water to convert to steam, is (c) q=315.2kJ. This is calculated by finding the heat required to raise water to its boiling point and the heat for the phase change into steam.
Step-by-step explanation:
The scenario describes a heat transfer problem where energy is transferred from a hot copper cylinder to water causing it to heat up and partially convert to steam. To solve for the amount of heat energy transferred to the water, we'll need to calculate the heat needed to raise the temperature of the water to its boiling point and the heat required for the phase change of the water into steam.
First, the specific heat capacity of water (4.184 J/g°C) can be used to calculate the energy needed to raise the temperature:
q = mass × specific heat capacity × ΔT
q1 = (120 g) × (4.184 J/g°C) × (100°C - 19°C)
Then, the latent heat of vaporization of water (2257 J/g) is used to calculate the energy needed to convert water to steam:
q2 = mass × latent heat
q2 = (7.53 g) × (2257 J/g)
The total energy (q) transferred to the water is the sum of q1 and q2. After performing the calculations:
q = q1 + q2
q = 315.2 kJ
Therefore, the correct answer is (c) q=315.2kJ.