Specific Heat of a Metal
Specific Heat of a Metal Post-Lab
I. Purpose
The purpose of this lab is to determine the specific heat of an unknown metal.
II. Safety
Wear goggles and lab apron at all times. Use caution when boiling water. Do not pick up hot beaker or hot metal with hands. Use tongs.
III. Pre-Lab Questions
1. A 12.5 g metal is raised to 100C in boiling water. It is put into 82.8 g of water at 22.4C, and the water rises to 28.6C. Recalling that the specific heat of water is 4.18J/gC, use the equation above to solve for the specific heat of the metal.
(12.5)(x)(71.4)=(82.5)(4.18)(6.2)
2.4=J/gC
IV. Procedure
First you will fill a 250 mL beaker with water then put it on the hot plate. Second you will mass and record the mass of a metal sample. Make sure you also record the metal's number. Gently place the metal sample in the beaker using tongs. While waiting, set your calorimeter. Put the calorimeter on the balance, zero it out, and fill it with 5/8 full of water. Record exact amount. Start a new experiment of the data collection system, and the temp of the water in the calorimeter as the water's initial temp. After the water has boiled for a while, use tongs to remove and quickly place it in the calorimeter. Put lid back on. Swirl the calorimeter and observe the temp every 15 secs until it drops. Record the max. temp as your final temp for both the water and metal. If you have time, do it over again!
V. Data & Observations
T initial
T final
Mass
Specific Heat
Trial 1
Metal #
100 C
20.2 C
70.5 g
-.102 j/g C
Water
19.1 C
20.2C
125.99 g
4.18 j/g C
Trail 2
Metal #
100 C
22.2 C
70.5 g
-.185 j/g C
Water
20.2 C
22.2 C
125.01 g
4.18 j/g C
VI. Calculations & Analysis
a. What was the temperature change of the metal?
20.2-100= -79.8 C
b. What was the temperature change of the water?
20.2-19.1= 1.1 C
c. Use the formula in the background information to solve for the specific heat of the metal.
Water (4.18)(125.99)(1.1)= Metal
I. Purpose
The purpose of this lab is to determine the specific heat of an unknown metal.
II. Safety
Wear goggles and lab apron at all times. Use caution when boiling water. Do not pick up hot beaker or hot metal with hands. Use tongs.
III. Pre-Lab Questions
1. A 12.5 g metal is raised to 100C in boiling water. It is put into 82.8 g of water at 22.4C, and the water rises to 28.6C. Recalling that the specific heat of water is 4.18J/gC, use the equation above to solve for the specific heat of the metal.
(12.5)(x)(71.4)=(82.5)(4.18)(6.2)
2.4=J/gC
IV. Procedure
First you will fill a 250 mL beaker with water then put it on the hot plate. Second you will mass and record the mass of a metal sample. Make sure you also record the metal's number. Gently place the metal sample in the beaker using tongs. While waiting, set your calorimeter. Put the calorimeter on the balance, zero it out, and fill it with 5/8 full of water. Record exact amount. Start a new experiment of the data collection system, and the temp of the water in the calorimeter as the water's initial temp. After the water has boiled for a while, use tongs to remove and quickly place it in the calorimeter. Put lid back on. Swirl the calorimeter and observe the temp every 15 secs until it drops. Record the max. temp as your final temp for both the water and metal. If you have time, do it over again!
V. Data & Observations
T initial
T final
Mass
Specific Heat
Trial 1
Metal #
100 C
20.2 C
70.5 g
-.102 j/g C
Water
19.1 C
20.2C
125.99 g
4.18 j/g C
Trail 2
Metal #
100 C
22.2 C
70.5 g
-.185 j/g C
Water
20.2 C
22.2 C
125.01 g
4.18 j/g C
VI. Calculations & Analysis
a. What was the temperature change of the metal?
20.2-100= -79.8 C
b. What was the temperature change of the water?
20.2-19.1= 1.1 C
c. Use the formula in the background information to solve for the specific heat of the metal.
Water (4.18)(125.99)(1.1)= Metal