Chemistry Lab
Chemistry Lab

Aim: To investigate the specific heat capacity of water, copper and aluminium by using a caloriometer.
Results:
1. Ohms Law: I=v/r, equation 3 = E=vlt hence you get E= v2t/r when ohms law is applied to equation 3. 2. De ionized water is used as it is the purest form of water, as it doesn’t contain ions from the soil like normal water which allow the conduction of electricity as normal water allows electrons to flow, thus preventing any extraneous variables to affect the experiment. 3. The value for Tf = 100o as water has a boiling point of 100o 4. SH = 1.00cal.g-1.c-1 m= density x volume (Tf – Ti) = 100 – 19.9 = 1 x 1,000ml = 80.1 = 1,000g
EH2O = SH.m.(Tf – Ti)
= 1 x 1,000 x 80.1
= 80,100cal Converting to Joules (1cal = 4.184j)
1000*4.184* 80.1= 335,138.4 joules g-1 deg-1

EKettle= V2.t / R V= 240 t= 219s R= 34.7
2402 * 219/34.7 =363,527.38 joules = E of kettle 5. The amount calories required to raise 1 gram of water by 1 degree Celsius is specific heat. Hence 80,100 calories are required to heat up the water, this shows the association between question 4. 6. In question 4, it can be observed that the energy produced by the kettle was 363,527.38 joules, however only = 335,138.4 joules g-1 deg-1 of energy was required to raise the water 80.1 degrees Celsius. Thus indicating that 23,388.38 joules of energy were lost, this could have occurred as a result of the kettle may have not been insulated appropriately, hence dissipation of heat or energy expenditure in order to heat up the kettle. 7. Initial temperature of Aluminium block = 100degrees Celsius
Final temperature of the water after Al block was placed inside = 23.8degrees Celsius
Initial