How much ice (in grams) would have to melt to lower the temperature of 354 ml of water from 26? c to 6? c? (assume the density of water is 1.0 g/ml.) ?

Heat gained in a system can be calculated by multiplying the given mass to the specific heat capacity of the substance and the temperature difference. It is expressed as follows:

Heat = mC (T2-T1)

When two objects are in contact, it should be that the heat lost is equal to what is gained by the other. From this, we can calculate things. We do as follows:

Heat gained = Heat lost

mC (T2-T1) = - mC (T2-T1)

C (liquid water) = 4.18 J/gC

C (ice) = 2.11 J/gC

(354 mL) (1.0 g/mL) (4.18 J/gC) (26 C - 6 C) = m (2.11 J/gC) (6 - 0C)

m = 2337.63 g of ice