data analysis for general chemistry introduction
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Data Analysis for General Chemistry
Introduction
Contact Information
Dr. Randa Roland
UCSC: 459-5486 Thimann 317
e-mail: [email protected]
website:chemistry.ucsc.edu course homepage
syllabus, powerpoints, etc.
General ProceduresCome to lab on time and prepared
Complete prelab Appropriate attire
Lab writeups due the following lab session Late lab penalty 25% off for each day late All writeups must be turned in no matter what
Makeup labs Same week or following week only See me and your TA
Prelab includes:
Title and date
Definitions
Answers to prelab questions
Procedure*
Data tables
Prelabs are done PRIOR to lab in your notebook
TA must sign off at start of lab session
Summary includes:
Title and date
Results (tables, graphs, values, errors, etc.)
Primary souces of errors
Sample calculations
Summaries are due one week after lab completion
Templates/guides are available (manual and web)
Lab Reports Includes:
Abstract
Results/sample calculations
Discussion/conclusions
Answers to postlab questions
Write-ups must be neat
Your TA decides whether your work is acceptable
Grading rubric is a guideline for you
Equation/Concept List
At the end of lab notebook, divide page(s) in half vertically
For each lab:
Left side: List primary equation(s) used
Define symbols Right side: Indicate linked concept
Example: M V = mol Finding moles of reactant M:
molarity (mol/L) or product in solutions
V: volume (L) Reactants and products are mol: moles related through mole ratio
Data Measurement
How do we record data?
What is the best value to report?
What is uncertainty (precision)?
Precision, Accuracy, Error
Precision: reproducibility
Accuracy: trueness
Error: standard deviation (uncertainty)
Accuracy vs. Precision
Precise
Not Accurate
Better Accuracy
Not PrecisePrecise
Accurate
Types of Error 1
Systematic: Accuracy
Trial Mass (g)1 10.222 10.233 10.194 10.175 10.22
Mass of Water
9.90
10.00
10.10
10.20
10.30
1 2 3 4 5
Trial
Mas
s (g
)
Types of Error 2
Random: Reproducibility / precision
Trial Mass (g)1 10.022 10.033 9.994 9.975 10.02
Mass of Water
9.80
9.90
10.00
10.10
10.20
1 2 3 4 5
Trial
Mas
s (g
)
Reporting Data
Average:
n
xxxx n21
Standard deviation:
1-n
x-xx-xx-x2
n
2
2
2
1
Examples of Precision
100 150 200 140 150 160 149 150. 151 149.5 150.0 150.5 149.9 150.0 150.1
and so on…
Average: “150”
Precision: very different
Examples of Precision/Standard Deviation 100 150 200 ± 50 140 150 160 ± 10 149 150. 151 ± 1 149.5 150.0 150.5 ± 0.5 149.9 150.0 150.1 ± 0.1
and so on…
Average: “150”
Standard deviation: reflects measuring device
Reporting Data Example
3
99.903.0100.01V
mL
Trial #
Volume (mL)
1 10.002 9.993 10.03
mL10.01V mL006666.10
Example continued
1- 3
9.99-10.0110.03-10.0110.00-10.01 2222 mL
mL0.02σ mL021213.0
Trial #
Volume (mL)
1 10.002 9.993 10.03
Average 10.01
Example continued
Report:
10.01 ± 0.02 g
%2.0%100g 10.01
g 0.02 error relative
Trial #
Volume (mL)
1 10.002 9.993 10.03
Average 10.01
Significant Figures
Which numbers are meaningful?
1. Mathematical
2. Standard Deviation
Mathematical Sig. Figs.
Multiplication/Division:
Round answer to fewest sig. figs.
Addition/Subtraction:
Round answer to fewest decimal places.
Standard deviation takes precedence over these rules.
Example
3 sig. figs./2 decimal places4 sig. figs./2 decimal places
Trial #
Volume (mL)
1 10.002 9.993 10.03
Average 10.01St. Dev. 0.02
Standard deviation takes precedence
Report: 10.01 ± 0.02 mL
Direct vs. Derived Values
Direct:
Measured /no calculations required
Derived:
Must be calculated from data
How do we account for our uncertainty?
Uncertainty in Measuring Devices
0 1 2
Ruler
1.38 cm ± 0.01 cm
Uncertainty in Measuring DevicesGraduated
cylinders
0.364 ± 0.001 mL
3.60 ± 0.01 mL
0.3
0.4
3
4
Error Propagation / Calculated Values
Addition:
)()()()( baba BABA
Subtraction:
)()()()( baba BABA
Standard deviations are additive
Error Propagation
Multiplication
BAABABBA ba
ba
)()())((
Division
BAB
A
B
A
B
A ba
b
a
)(
)(
Relative errors are used
Addition
12.5 g = 0.1 g
+ 2.05 g = 0.01g
12.55 g = 0.11 gReport: 12.6 ± 0.1 g
Subtraction
12.5 g = 0.1 g
– 2.05 g = 0.01g
10.45 g = 0.11 gReport: 10.4 ± 0.1 g
Multiplication
12.5 cm = 0.1 cm
2.05 cm = 0.01cm
25.625 cm2 = ?
Report: 25.6 ± 0.3 cm2
= 25.625 cm2
0.1 cm
12.5 cm
0.01 cm
2.05 cm
+ = 0.33 cm2
Division 12.5 g = 0.1 g
2.05 cm3 = 0.01cm3
6.09756 g = ? cm3
Report: 6.10 ± 0.08 g/cm3
= 6.09756 g
cm3
0.1 g 12.5 g
0.01 cm
2.05 cm
+ = 0.0785g/cm3
Example sidecirclecylinder LAV
diameter, d
length, l
lddldldV
ldldlrV
ldd
ld
22
222
44
44
Measured: diameter
length
Example Density = mass/Volume
)()(
)(4
4
2
2 ld
m
ld
m
ld
mD
lddmld
m
ld
mD lddm
22
44
diameter, d
length, l
Measured: mass
diameter
length
Density Calculation
A 218.44 ± 0.01 g metal cylinder has diameter of 2.50 ± 0.01 cm and is 5.00 ± 0.01 cm long.
What is the density of the metal?
Mass: 218.44 ± 0.01 g Diameter: 2.50 ± 0.01 cm Length: 5.00 ± 0.01 cm
Volume = ¼d2l Density = m/V
Density of a Cylinder
3290005.8
)00.5()50.2(
)44.218(4
cm
g
cmcm
gD
lddmld
m
ld
mD lddm
22
44
Formula:
Density:
Density continued
Standard deviation:
Report: D = 8.90 ± 0.02 g/cm3
33
3
0182.0002046.090005.8
00.5
01.0
50.2
01.0
50.2
01.0
44.218
01.090005.8
cm
g
cm
g
cm
cm
cm
cm
cm
cm
g
g
cm
gD
Final answer:
Density of a cylinder, take 2
32 5437.24)00.5()50.2(4
cmcmcmV
Volume: 24.5 ±0.2 cm3
Standard deviation:
33
3
24544.001.05437.24
00.5
01.0
50.2
01.0
50.2
01.05437.24
cmcm
cm
cm
cm
cm
cm
cmcmV
Volume:
Density continued
333
3
30732.0008209.09159.8
5.24
2.0
44.218
01.09159.8
cm
g
cm
g
cm
cm
g
g
cm
gD
339159.8
5.24
44.218
cm
g
cm
gD
Note difference: D = 8.90 ± 0.07 g/cm3
Volume: 24.5 ±0.2 cm3
Mass: 218.44±0.01 g
VmV
m
V
mD Vm
Standard deviation:
Density:
Summary
Multiple measurements required
Average
Standard deviation
Direct uncertainty: device dependent
Calculated uncertainty: error propagation
Review sig. fig. rules
Graphing / Visualizing Data
Volume (mL) Mass (g)5.00 4.93
10.00 9.6215.00 14.9920.00 21.0225.00 24.8930.00 29.77
Density of Water
Density of Water
y = 1.0028x
0
10
20
30
0.00 10.00 20.00 30.00
Volume (mL)
Mas
s (g
)
OHdensitymL
g
xx
yylope
20028.1s
12
12
Graphing
For a plot of mass vs. volume
y-axis: mass in g
x-axis: volume in mL
mL
gdensity
volume
masslope 00.1s
Density: linear relationship of mass to volume
Densities
Substance Density
(g/mL)
wood 0.35
water 1.00
quartz 2.65
diamond 3.51
Ti 4.5
Ag 10.5
Au 19.3
Os 22.4
Increasing density
=
Increasing “heaviness”