1. Purpose
The purpose of this lab was answered in 4 questions, and their answers are here shown. The density of the metals we used were 5g/cm3. The density of a metal piece does not depend on its size, it depends on the total mass and total volume. The most accurate way of determining density is dividing mass by volume. You can’t identify metals by their density. It can help you narrow the options down, but you can’t identify a metal by using only its density. 2. Question

Can we find out the density of a metal only using water?
3. Variables
Independent Variable(s): Temperature (27ºC); Mass (5g)
Dependent Variable: Density of Metals
4. Pre-Lab Questions
a) 43 cm3
b) 73 cm3
1. 30 cm3
2. 3.43 cm3
3. Its density is 7.131 g/cm3
5. Materials
Metal A (Zinc)
50cm3 measuring cylinder
25cm3 measuring cylinder
250cm3 beaker
Glass Water
Tap Water
Balance
6. Procedure
Find the mass of the watch glass
Put the copper piece on the watch glass and find their mass
Fill a 50cm3 graduated cylinder with enough water that you think will completely cover Metal A and record this volume in the data table Fill a 25cm3 graduated cylinder with enough water that you think will completely cover Metal A and record this volume in the data table Fill a 250cm3 beaker with enough water that you think will completely cover Metal A and record this volume in the data table Carefully slide Metal A down the side of the 50cm3 graduated cylinder so as to not crack the bottom of the cylinder. Record the volume of the water with Metal A submerged in it Empty the graduated cylinder, dry off Metal A, and repeat steps #1-4 for the other cylinder and the beaker Complete the calculations 1 and 2, then report those amounts. Also record your mass on the class data table. 7. Data

50cm3 measuring cylinder
25cm3 measuring cylinder
250cm3 beaker
Mass of Metal
5g ; 5g ; 5g
5g ; 5g ; 5g
5g ; 5g ; 5g
Volume of Water Alone
20cm3 ; 20cm3 ; 20cm3
20cm3 ;...

...3
Density of MetalLab
I. Purpose and Procedure
In this experiment, groups were each given two unknown metals in which they had to find the mass, volume, and density. After finding the density of the unknown metals by dividing the mass by the volume, the groups had to exchange data and find the average densities of the two unknown metals. A table of accepted value of metals and their densities was given out to each group so they could match the average densities to the accepted values and identify what they unknown metals were.
The objective of this lab was to determine the identity of unknown metals by calculating their densities, and to determine a graphical relationship between the mass and volume of a given substance.
Each group was given two unknown metals, a 100 mL graduated cylinder, a balance, and a weighing boat. To find the mass, the experimenters had to weigh the empty weighing boat. After, they had to weigh the unknown metal in the boat. Then, they had to subtract the mass of the weighing boat from the mass of unknown metal to figure out just the mass of the metal. To find the volume, the experimenter filled up the graduated cylinder to 50 mL. Then, they added the...

...the densitylab unknown metals were weighed using beakers filled with water and an electronic scale. First the metal objects were weighed using an electronic scale. Then using water, the beakers were filled half way. Next, the metal objects were poured in. Then the amount of how much the water rose after the metal was put in is checked. Lastly, record the data and clean the objects used and put away.
Design
Research question: If mass and volume are correctly measured can the density of an unknown metal be calculated.
Variables:
Controlled: Water, Electronic Scale, Graduated Cylinder
Dependent: Density; Mass and Volume
Independent: Metal(s)
Method
Apron, Goggles, Electronic Balance, Beaker, Graduated Cylinder, water, unknown metal samples
Labeled Diagram
Uncertainties: Electronic Balance ± 0.01g
Hexagon ± 0.0mL Graduated Cylinder ± 1.0 mL
The independent variable is measured based off the how much the water rises.
The dependent variable is measured when the Initial Volume is subtracted from the final volume, which gives the density of the metal sample.
Controlling the Controlled Variables: The water and electronic scale were controlled. These materials were controlled because the amount of water put into the graduated cylinder could differ,...

...Chemistry
Period 7
9/17/13
The Density of MetalsLab
BACKROUND: Density is a constant relationship between the mass and volume of a specific type of matter. Measurements of both mass and volume can be obtained for a metal sample. The relationship can be shown graphically by plotting the volume of a sample on the horizontal x-axis and the mass of the sample along the vertical y-axis. Plotting the values for several samples, a linear relationship can be seen for a density (slope=density).
PURPOSE: During this lab, you will investigate several questions about density. 1) What are the densities of metals A and B? 2) Does the density of a piece of metal depend on its size? 3) According to percent error calculations, which of the methods of determining density is the most accurate? 4) Can you identify the metals by their densities?
PRE-LAB QUESTIONS: 1) The volume of the water in the cylinder below is 43mL.
2) The volume of the metal shot and the water in the graduated cylinder is 73mL.
3) The volume of the metal added to the graduated cylinder is 29mL.
MATERIALS:
- Metal cylinders - Graduated cylinders - Calculator
- Water - Electric Balances
SAFETY: No metals should be...

...Density of Metals
Problem: How does the mass and volume help determine the density of known metal samples?
Hypothesis: When comparing the density of Zn(zinc) and Cu(copper), you will find that Copper is more dense than Zinc. You can test this out by using the density formula D=m/v.
Materials:
* 2 metals (options: zn, al, or cu)
* 3 samples of each metal (small, medium, and large)
* Scale/Balance
* Calculator
* Water
* Graduated Cylinder
Safety:
* Be prepared for your work in the laboratory.
* Read all procedures thoroughly before entering the lab and/or starting experiment.
* Be alert and proceed with caution at all times in the lab.
Step by Step Procedure:
1. Wash hands with soap and water
2. Grab all materials and set them out
3. Pick one metal out of the two you have chosen to compare and get your three samples (small, medium, large)
4. Find the mass of each sample using a scale/balance and then find the volume (using a graduated cylinder filled with water and putting each sample in the filled graduated cylinder to determine the volume)
5. Create a data table and write all the information collected down
6. Repeat steps three-six with the second metal of your choice
7. On logger pro, plug in all needed information to make a graph for...

... 9/16/14
Physics 01L
Density
Abstract
This experiment was conducted in order to determine the density of the Aluminum metal samples provided in the lab. Specific tools such as the vernier caliper and balance scale were used to measure and record the values found. Given that density is a measurement of mass over volume, both of these quantities would have to be determined experimentally, prior to proceeding with the calculation of the density, for each of the six subjects tested. Being as accurate and precise as possible, the data yielded a density that was similar to that of the accepted value for the density of aluminum. Taking averages of the measurements recorded by both partners may have introduced a variable for error. However, upon calculating the percent error of the results found, it was concluded that there was less than a three percent error, which supported the accuracy and credibility of the experiment.
Data
Table 1: Tabular Presentation
Aluminum
Diameter D1 (cm)
Diameter
D2 (cm)
Average
Diameter (cm)
Height
H1 (cm)
Height
H2 (cm)
Average Height (cm)
Mass (g)
Volume
(cm3)
1
1.27 cm
1.27 cm
1.27 cm
1.55 cm
1.548 cm
1.549 cm
5.6 g
V=1.96cm3
2
1.26 cm
1.266 cm
1.263 cm
2.64 cm
2.64 cm
2.64 cm
9.6 g
V=3.31 cm3
3
1.26 cm
1.266 cm
1.263 cm
4.726 cm
4.728 cm
4.727 cm
16.6 g...

...Ashley Robins
9/13/11
Honors Chemistry
Period 4
DensityLab
Purpose:
1. To determine the density of a solid using different laboratory techniques for measuring volume.
2. To use the intensive property of density to identify an unknown substance.
Procedure:
1. Obtain a bag marked with a number containing a cube and a cylinder from the teacher. Record the number on the bag in the data table.
Density of a cube:
Using a balance, record the mass of the cube to the nearest tenth of a gram. Then measure the length, width and height of the cube to the nearest hundredth of a cm. Last, calculate the volume of a cube using the formula L x W x H.
Density of a cylinder by water displacement:
Using a balance, record the mass of the cylinder to the nearest tenth of a gram. Then fill a graduated cylinder of water about half full. Record the volume to the nearest tenth of a mL. After that you carefully drop the cylinder in the graduated cylinder and record the new volume of water to the nearest tenth of a mL. The last thing you do is subtract the volume of the water you had at the beginning from the volume of water you had after adding the cylinder. This number is the volume of your cylinder.
Data:
Cube Cylinder
Mass of cube:10.4g Mass of cylinder: 29.1g
Length of cube:2.50cm...

...Lab No.1: density, accuracy and precision
Aim: to determine the relative precision and accuracy of different glassware items by calculating the density of a known substance.
Introduction: the density of a substance is its mass per unit volume. (where P-density, m- mass and v- volume). Different materials usually have different densities and densities vary according to the pressure, temperature and purity of a substance. When measuring, there is always a small uncertainty or error and therefore no measurement is exact.
Variables:
Independent: the type of liquid used
Dependant: the volume and density of the liquid
Controlled: the same type of beaker as the mass of the beaker is never changed
Hypothesis : the larger the divisions on the glassware items the bigger the percentage of error.
Materials:
Car oil
Coke Zero
Liquid soap
Salty water
1x 200ml beaker
1 x 100ml beaker
1 x 10ml cylinder
1 x weighing scale
1 x thermometer
Procedure:
1. Weigh a dry 100 ml beaker, a 10 ml graduated cylinder and a 10 ml pipette (in this case weigh a 150 ml beaker that you will transfer into a pipette, pipettes cannot be weighted effectively) and record the mass for each case. Do not forget that trailing zeros are significant figures and should be recorded.
2. Obtain a fair amount of water and measure its temperature.
(Remember here some students...

...Density of a regular shaped object
Object Mass / g
± 0.05 g * Length / cm
± 0.003 cm ** Width / cm
± 0.003 cm ** Height / cm
± 0.003 cm **
T1 T2 T3 T4 T5 T1 T2 T3 T4 T5 T1 T2 T3 T4 T5
A 44.9 5.975 5.980 5.980 5.980 5.975 1.500 1.500 1.500 1.500 1.500 0.600 0.600 0.605 0.600 0.600
B 16.5 4.400 4.395 4.400 4.395 4.395 1.500 1.500 1.495 1.500 1.495 0.300 0.305 0.305 0.300 0.300
C 22.5 3.000 2.995 3.000 3.000 3.000 1.500 1.505 1.495 1.500 1.500 0.600 0.595 0.600 0.595 0.595
D 22.6 6.005 6.000 6.010 6.005 6.000 1.500 1.500 1.495 1.500 1.495 0.295 0.300 0.300 0.305 0.300
E 11.4 3.040 3.045 3.040 3.075 3.070 1.500 1.495 1.500 1.500 1.495 0.300 0.300 0.305 0.300 0.300
F 5.80 1.550 1.550 1.540 1.550 1.550 1.495 1.500 1.500 1.495 1.500 0.300 0.300 0.300 0.300 0.300
Table 1: Raw data table
Half the smallest division: 0.1 ÷ 2 = 0.05 g
** Half the smallest division: 0.005 ÷ 2 = 0.0025 ≃ 0.003 cm
Inaccurate set of data due to random error. (See Evaluation)
Table 2: Data processing 1
Object Mass / g
± 0.05 g Average L / cm Abs. Unc. L / cm Average W / cm Abs. Unc. W / cm Average H / cm Abs. Unc. H / cm
A 44.9 5.98 0.006 1.50 0.003 0.60 0.007
B 16.5 4.40 0.006 1.50 0.006 0.30 0.006
C 22.5 3.00 0.007 1.50 0.008 0.60 0.006
D 22.6 6.00 0.009 1.50 0.006 0.30 0.008
E 11.4 3.06 0.03* 1.50 0.006 0.30 0.007
F 5.80 1.55 0.02* 1.50 0.006 0.30 0.003
Since the uncertainties can only be written with 1 s.f, the number of decimal places cannot...

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