Final answer:
To find the final temperature after adding 65.0 kilojoules to 150g of water at 0.0°C, we use the specific heat capacity of water and the formula ΔT = q/(mc). The calculation gives us a final temperature around 103.6°C, assuming no phase change occurs.
Step-by-step explanation:
To determine the final temperature after adding 65.0 kilojoules of energy to 150g of water at 0.0°C, we use the specific heat capacity of water. The specific heat capacity is the amount of heat energy required to raise the temperature of one gram of a substance by one degree Celsius. For water, this value is typically 4.18 joules per gram per degree Celsius (J/g°C). First, we need to convert the energy from kilojoules to joules: 65.0 kJ = 65,000 J.
The formula to calculate the change in temperature is:
q = mcΔT, where q is the heat energy transferred, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Solving for ΔT, we have: ΔT = q / (mc) = 65,000 J / (150g × 4.18 J/g°C) ≈ 103.6°C
Since the initial temperature is 0.0°C, the final temperature would be approximately 103.6°C.