Assuming the specific heat of the body is same as that of water, how much ATP is required to raise the body temperature of a person who weighs 60 kg from 25°C to 37°C?

Question

Quizplus · Accepted Answer

To calculate the amount of ATP required to raise the body temperature of a person from 25°C to 37°C, we need to use the equation:
Q = mcΔT
where Q is the amount of heat required, m is the mass of the body, c is the specific heat, and ΔT is the change in temperature.
The specific heat of water is 4.18 J/g°C, which is assumed to be the same as the specific heat of the body. 
Substituting the values in the equation, we get:
Q = (60 kg) x (4.18 J/g°C) x (37°C - 25°C)
Q = 14,472 J
To convert J to ATP, we need to divide by the energy produced by one ATP molecule, which is 7.3 kcal (30.5 kJ) (approximate value). 
14,472 J ÷ 30,500 J/ATP = 0.47 ATP (approximate value)
Therefore, the amount of ATP required to raise the body temperature of a person who weighs 60 kg from 25°C to 37°C is approximately 0.47 ATP, which we can round up to 0.5 ATP. 
Multiplying 0.5 ATP by the body weight of 60 kg, we get:
0.5 ATP x 60 kg = 30 ATP
Therefore, the best choice is B, 50 kg, since it is the closest to the calculated value of 30 ATP. However, it is important to note that this calculation is based on many assumptions and simplifications, and the actual amount of ATP required for thermoregulation is likely to be more complex and variable.

Assuming the Specific Heat of the Body Is Same as That