Question

If you drink 4.5 glasses of ice water at 0.0°C, how much heat energy in kilojoules is transferred as this water is brought to body temperature? (Assume each glass of water contains 250.0 g of water and that your body temperature is 37°C).

Answer 1

Approximately 174.2 kJ of heat energy is required to bring 4.5 glasses of ice water at 0.0°C up to body temperature (37°C).

Step-by-step explanation:

To calculate the heat energy transferred as 4.5 glasses of ice water at 0.0°C are brought to body temperature (37°C), we use the specific heat capacity of water and the mass of water consumed. The specific heat capacity for water is approximately 4.186 joules per gram per degree Celsius (J/g°C), and a glass of water is given as 250.0 g. Multiplying the mass by the change in temperature (ΔT = 37°C - 0°C = 37°C) and the specific heat capacity gives us the heat energy per glass.

The calculation for one glass would be:

• Heat energy = mass × specific heat capacity × ΔT
• Heat energy = 250.0 g × 4.186 J/g°C × 37°C
• Heat energy = 38,686.5 J or 38.7 kJ (rounded to one decimal place)

For 4.5 glasses, we multiply the heat energy for one glass by 4.5:

• Total heat energy = 38.7 kJ × 4.5
• Total heat energy = 174.15 kJ

Therefore, approximately 174.2 kJ of heat energy is transferred when 4.5 glasses of ice water are brought to body temperature.