06.03 Calorimetry Essay Example

06.03 Calorimetry: Lab Report
Procedure:
Part II: Determining the Specific Heat of an Unknown Metal
Data and Observations:
Part I: Determining the Specific Heat of a Known Metal
Metal:
Aluminum
Zinc
Iron
Copper
Mass of metal
27.776g
41.664g
34.720g
41.664g
Volume of water in the calorimeter
26.0mL
26.0mL
26.0mL
26.0mL
Initial temperature of water in calorimeter
25.3 °C
25.3 °C
25.3 °C
25.3 °C
Temperature of hot water and metal in hot water bath
100.5 °C
100.5 °C
100.5 °C
100.5 °C
Final temperature reached in the calorimeter
31.6 °C
34.8 °C
33.1 °C
34.5 °C
Observations: The hottest temperature reached was Zinc at 34.8°C & Copper was the heaviest metal

Part II: Determining the Specific Heat of an Unknown Metal
Metal:
Metal A
Metal B
Metal C
Mass of metal
15.262g
25.605g
20.484g
Volume of water in the calorimeter
24.0mL
24.0mL
24.0mL
Initial temperature of water in calorimeter
25.2 °C
25.3 °C
25.2 °C
Temperature of hot water and metal in hot water bath
100.3 °C
100.3 °C
100.3 °C
Final temperature reached in the calorimeter
27.5 °C
32.2 °C
28.0 °C
Observations: The heaviest metal was Metal B. The metal with the highest temperature was Metal B

Calculations:
Show your work and write a short explanation with each calculation.
Part I:
1. Calculate the energy change (q) of the surroundings (water) using the enthalpy equation

qwater = m × c × ΔT.

We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. qwater = m × c × ΔT m = mass of water = density x volume = 1 x 26 = 26 grams ΔT = T(mix) - T(water) = 38.9 - 25.3 = 13.6 q(water) = 26 x 13.6 x 4.18 q(water) = 1478 Joules

The water has absorbed the heat of the metal. So, qwater = qmetal

2. Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation.