Download Experiment SHC metal and water

Experiment - 1.
14th Nov. 2011
Specific Heat Capacity
Objectives;
To set up the apparatus safely and ensure the setup is stable.
To understand that thermal equilibrium is reached when the final temperature is constant.
To use the formula Q = mc
Aim: To determine the specific heat capacity c of a metal
Apparatus:
 unknown metal sample
 thread
 retort stand
 calorimetre (or styrofoam cup)
 thermometer
 cloth or tissue paper
 measuring cylinder (150-200 cm3)
 beaker (250-500ml)
 stirrer
 electronic balance
 electrical kettle
 water
 lid with holes for thermometer
Procedure;
1. Measure and record the mass m of the metal sample using the electronic balance.
2. Tie the metal sample with a piece of thread and suspend it in a beaker of water. Suspend a
thermometer alongside the metal sample but make sure they do not touch. Ensure that both the
sample and the thermometer are fully immersed in water but not touching the base of the beaker.
Cover the beaker with the lid.
3. Start heating the beaker and its contents using the Bunsen burner. After the water has boiled
for a few minutes, take the temperature T1 of the boiling water. This temperature T1 is the initial
temperature of the metal. Slowly remove the thermometer but not the metal sample.
4. Add 100ml of tap water to the calorimeter cup. Measure and record the initial temperature T 2 of
the tap water.
5. Remove the metal sample from the beaker of boiling water. Dry it quickly with a piece of cloth or
tissue paper and transfer it into the tap water in the Styrofoam cup. The water should cover the
metal completely.
6. Stir the water in the Styrofoam cup. Measure and record the highest temperature T3 reached.
This is the equilibrium of the metal and the water.
Readings
Mass of iron sample m
( g )
Mass of 100 ml of water
Initial temperature of iron sample T1 (
Initial temperature of tap water T2 (
=
)
)
Final temperature of iron and tap water T3 (
Specific heat capacity of water
)
=
Guiding questions;
1. Why the calorimetre covered by styrofoam?
2. State the reason for stirring the water in the calorimetre when the heated iron sample is
placed inside?
3. Is your answer for the specific heat capacity c of the metal likely to be an overestimation
or underestimation? Why?
4. How do you ensure that minimal thermal energy from the hot metal is lost to the
surroundings? Comment on the amount of water, choice of container, stirrer and lid used
in the experiment.