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.