Answer:
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
