Calculate the heat lost by the hot water using your results for Experiment 3: Measuring the Enthalpy of Fusion of Water. Heat must be expressed in kilojoules (kJ). Q = (4.18 J/g °C) x (1 kJ/1000 J) x mass of water (g) x ΔT

7.399 kJ

Explanation:

The heat lost (Q) by the hot water is the product of the mass (m) of hot water, temperature difference (ΔT) and the (c) specific heat capacity of water. Mathematically,

Q = m*c*ΔT

The final volume of hot water = 30 ml, and the density of water = 1 g/ml

Thus, mass (m) = 30*1 = 30g

ΔT = final temperature - initial temperature = 60 - 1 = 59 °C

Specific heat capacity of water = 4.18 J/g °C

Therefore

Q = m*c*ΔT = 4.18*30*59 = 7398.6 J

To convert from J to kJ, we will divide by 1000:

Q = 7398.6/1000 = 7.399 kJ