Final answer:
The heat energy required is calculated using the formula q = mcΔT, where m is 100.0 g (from 100.0 ml of water) and ΔT is 33 °C (the temperature increase from 4.0 °C to 37 °C). With a specific heat capacity of 4.18 J/g°C for water, the required energy is 13794 J, which does not match any of the given answer options.
Step-by-step explanation:
To calculate the amount of heat energy required to raise the temperature of 100.0 ml of water from 4.0 °C to 37 °C, we can use the formula for heat transfer: q = mcΔT, where q is the heat transferred, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature. Since the specific heat of water is 4.18 J/g°C and the density of water is approximately 1 g/ml, the mass of 100.0 ml of water is 100.0 g. Therefore, the calculation is
q = (100.0 g) × (4.18 J/g°C) × (37 °C - 4.0 °C)
q = 100.0 g × 4.18 J/g°C × 33 °C
q = 13794 J
However, options (a) through (d) do not match this result, which implies there might be an error in the answer choices or a misinterpretation of the question.