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

answer: a tank of height h is filled with water and sits on the ground. water squirts from a hole at a height y above the ground and has a range r. for two y values, 0 and h, r is zero. determine the value of y for which the range will be a maximum.

explanation: