Answer :
Final answer:
The correct option is B) 3700 calories.
Explanation:
To calculate the heat expended to warm the water, we can use the formula Q = mcΔT, where Q is the heat, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature. Given that ice-cold water of 100g is to be warmed from 5°C to 37°C:
Q = 100g * 4.184 J/g°C * (37°C - 5°C)
= 100g * 4.184 J/g°C * 32°C
= 13388.8 J
= 13.388 kJ.
Converting this to calories using 1 calorie = 4.184 J, we get 13.388 kJ * 1000 / 4.184
= 3206.1 calories.
Therefore, the correct option is B) 3700 calories.
