If a 375ml sample of water was cooled from 37.5 C to 0 C, how much heat was lost in joules?

To answer this item, we use 1 g/mL as the conventional density of water at any temperature. Thus, the amount of water in grams is,

m = (375 mL) x (1g/mL) = 375 g

Then, we use the equation

H = mcpdT

where m is the mass, cp is the specific heat of water (4.18 J/g°C), and dT is the temperature difference. Substituting,

H = (375 g) (4.18 J/g°C) (0° - 37°)

= - 57997.5°C

Therefore, the amount of heat released is equal to 57,997.5°C.