Background According to the First Law of Thermodynamics, energy can neither be created nor destroyed-it only changes from one form to another. In this experiment, the chemical energy stored in wax is converted into heat energy through combustion. However, part of this energy is absorbed by the copper vessel and lost to the surroundings, illustrating inefficiencies in energy conversion. Hypothesis If wax is burned under controlled conditions, the chemical energy released will increase the temperature of water and the copper vessel proportionally to their specific heats. Objectives To demonstrate the conversion of chemical energy into heat energy. To calculate the heat absorbed by the water and the copper vessel. To understand losses during energy transformation. Experiment Burn 10 g of wax under a copper vessel containing 100 g of water. Measure the rise in water temperature using a thermometer. Calculate heat energy absorbed. 1 mole of wax burning = 14800 kJ of energy releasedC25H52 molecule mass is 352g1 mole is 352g1 kg of wax = 2.841 mole1 kg of wax gives 42 MJ of energy1 g of wax gives 42 KJ of energy10 g of wax burning will give 420 KJ of energyNow to heat water from 25 degrees centigrade10 gm of water with Specific heat = 4.184 J is required to raise the temperature of 1 g of water by 1 degree100 g of water needs 418.4 J for each degreeIf it was only water, all of it would evaporate.But there is a copper vessel which is also getting heated up.Which needs 0.385 for 1 g of copper by 1 deg c Expected Outcomes The heat gained by water and copper will be less than 420 kJ, confirming energy losses to the environment. Significance The experiment highlights the principle of energy conservation and practical inefficiencies during energy conversion processes. Source : Science and Innovation for Sustainability - Activity Guide Book 2026 & 2027