M 1-6 Exams
.pdf
keyboard_arrow_up
School
Portage Learning *
*We aren’t endorsed by this school
Course
103
Subject
Chemistry
Date
Jan 9, 2024
Type
Pages
34
Uploaded by MinisterOctopusPerson886
Pay
it
forward.
MODULE
1
EXAM
Question
1
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
1.
Convert
845.3
to
exponential
form
and
explain
your
answer.
2.
Convert
3.21
x
105
to
ordinary
form
and
explain
your
answer.
1.Convert
845.3
=
larger
than
1
=
positive
exponent,
move
decimal
2
places
=
8.453
x
102
2.Convert
3.21
x
10*
=
negative
exponent
=
smaller
than
1,
move
decimal
5
places
=
0.0000321
Question
2
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Using
the
following
information,
do
the
conversions
shown
below,
showing
all
work:
1
ft
=12
inches
1
pound
=
16
oz
1
gallon
=
4
quarts
1
mile
=
5280
feet
1
ton
=
2000
pounds
1
quart
=
2
pints
kilo
(=
1000)
milli
(=
1/1000)
centi
(=
1/100)
deci
(=
1/10)
1.
24.6
grams
=
?
kg
2.
6.3ft="7inches
1.
24.6
grams
x
1
kg
/1000
g
=
0.0246
kg
2.
6.3ftx12in/1ft=75.6inches
please
always
use
the
correct
units
in
your
final
answer
Question
3
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Do
the
conversions
shown
below,
showing
all
work:
1.
28C=7°K
2.
158F
=7-C
3.
343K=7°F
1.
28C+
273
=301°K
°C
-
°K
(make
larger)
+273
2.
158F-32+1.8=70°C
°F
-
°C
(make
smaller)
-32
+1.8
3.
343°K-273=70°Cx1.8
+
32
=158°F
oK
-
°C
-
°F
Question
4
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Be
sure
to
show
the
correct
number
of
significant
figures
in
each
calculation.
1.
Show
the
calculation
of
the
mass
of
a
18.6
ml
sample
of
freon
with
density
of
1.49
g/ml
2.
Show
the
calculation
of
the
density
of
crude
oil
if
26.3
g
occupies
30.5
ml.
1.
M=DxV=149x18.6
=27.7¢
2.
D=M/V=26.3/30.5=0.862
g/ml
Question
5
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
1.
3.0600
contains
?
significant
figures.
2.
0.0151
contains
?
significant
figures.
3.
3.0600
+
0.0151
=
?
(give
answer
to
correct
number
of
significant
figures)
1.
3.0600
contains
5
significant
figures.
2.
0.0151
contains
3
significant
figures.
3.
3.0600
=+
0.0151
=
202.649
=
203
(to
3
significant
figures
for
0.0151)
Question
6
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Classify
each
of
the
following
as
an
element,
compound,
solution
or
heterogeneous
mixture
and
explain
your
answer.
1.
Coca
cola
2.
Calcium
3.
Chili
1.
Coca
cola
-
is
not
on
periodic
table
(not
element)
-
no
element
names
(not
compound)
appears
to
be
one
substance
=
Solution
2.
Calcium
-
is
on
periodic
table
=
Element
3.
Chili
-
is
not
on
periodic
table
(not
element)
-
no
element
names
(not
compound)
appears
as
more
than
one
substance
(meat,
beans,
sauce)
=
Hetero
Mix
Question
7
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Classify
each
of
the
following
as
a
chemical
change
or
a
physical
change
1.
Charcoal
burns
2.
Mixing
cake
batter
with
water
3.
Baking
the
batter
to
a
cake
1.
Charcoal
burns
-
burning
always
=
chemical
change
2.
Mixing
cake
batter
with
water
-
mixing
=
physical
change
3.
Baking
the
batter
to
a
cake
-
baking
converts
batter
to
new
material
=
chemical
change
Question
8
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Show
the
full
Nuclear
symbol
including
any
+
or
-
charge
(n),
the
atomic
number
(y),
the
mass
number
(x)
and
the
correct
element
symbol
(Z)
for
each
element
for
which
the
protons,
neutrons
and
electrons
are
shown
-
symbol
should
appear
as
follows:
*Z,+-»
31
protons,
39
neutrons,
28
electrons
31
protons
=
Gas;,
39
neutrons
=
*Ga.,,
28
electrons
=
(+31
-
28
=
+3)
—
70Ga31+3
Question
9
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Name
each
of
the
following
chemical
compounds.
Be
sure
to
name
all
acids
as
acids
(NOT
for
instance
as
binary
compounds)
1.
PF;s
2.
Al
(CO,),
3.
H.CrO.
1.
PF;
-
binary
molecular
=
phosphorus
pentafluoride
2.
Al(CO:s);
-
nonbinary
ionic
=
aluminum
carbonate
3.
H.CrO,
-
nonbinary
acid
=
chromic
acid
incorrect
fluoride
prefix
Question
10
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Write
the
formula
for
each
of
the
following
chemical
compounds
explaining
the
answer
with
appropriate
charges
and/or
prefixes
and/or
suffixes.
1.
Carbon
monoxide
2.
Manganese
(IV)
acetate
3.
Phosphorous
acid
1.
Carbon
monoxide
-
ide
=
binary,
mono
=10
=
CO
2.
Manganese
(IV)
acetate
-
Mn+,
C,H;0,*
=
Mn(C,H;0,).
3.
Phosphorous
acid
-
nonbinary
acid
of
H
+
phosphite
(PO;3)
=
H;PO;
MODULE
2
EXAM
Question
1
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Show
the
calculation
of
the
molecular
weight
for
the
following
compounds,
reporting
your
answer
to
2
places
after
the
decimal.
1.
Al(CO;);
2.
CHNO.CI
1.
2Al+
3C
+
90
=
233.99
2.
8C+6H+
N+
40
+
Cl
=
215.59
Question
2
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Show
the
calculation
of
the
number
of
moles
in
the
given
amount
of
the
following
substances.
Report
your
answerto
3
significant
figures.
1.
13.0
grams
of
(NH.).CO,
2.
16.0
grams
of
C;H:NO.Br
1.
Moles
=
grams
/
molecular
weight
=
13.0/96.09
=
0.135
mole
2.
Moles
=
grams
/
molecular
weight
=
16.0
/
260.04
=
0.0615
mole
Question
3
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Show
the
calculation
of
the
number
of
grams
in
the
given
amount
of
the
following
substances.
Report
your
answer
to
1
place
after
the
decimal.
1.
1.20
moles
of
(NH.).CO;
2.
1.04
moles
of
C;H:NO,Br
1.
Grams
=
Moles
x
molecular
weight
=
1.20
x
96.09
=
115.3
grams
2.
Grams
=
Moles
x
molecular
weight
=
1.04
x
260.04
=
270.4
grams
Question
4
Click
this
link
to
access
the
Periodic
Table.
This
may
be
helpful
throughout
the
exam.
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
Related Questions
2. Do the following calculations and use the correct number of significant figures in your answers. Assume all numbers are the results of measurements.
a. 0.208 + 4.9 + 1.11
b. 228 + 0.999 + 1.02
c. 8.543 − 7.954
d.(3.2 × 10−2) + (5.5 × 10−1) (hint: Write in the decimal form first, then add.)
e. 336.86 − 309.11
f. 21.66 − 0.02387
arrow_forward
Find the difference between the value of x2 and the sum of x1 plus x3.; let x4 be equivalent to the sum of x1 and x3 and let x5 be the difference between x2 and x5. This calculation scheme is shown below. Make notes about any similarities or differences between the values in your notes. x4 = x1 + x3 x5 = x2 – x4
Data Analyis
This section will include all data collected during the lab.
Thermochemical Data
Tinitial (°C)
Tfinal (°C)
ΔT (°C)
moles NaOH
qreaction (kJ)
ΔHrxn
Reaction 1
25.0
30.3
+5.3
0.025
-1.11
-44.4
Reaction 2
25.0
37.0
+12.0
0.025
-2.51
-100.4
Reaction 3
25.0
31.7
+6.7
0.025
-1.40
-56.1
Reaction 1: NaOH(s) → Na+(aq) + OH-(aq) + x1 kJ
1g /39.977g/mol = 0.025 moles
Moles NaOH = 0.025
qsolution = (4.184 J/g °C) (50.0g) (30.3°C -25.0°C)
= -1108.76 J/ 1000
qreaction (kJ) = -1.11 kJ
ΔH = -1.11 kJ/ 0.025 moles
ΔHrxn = -44.4 kJ/mol…
arrow_forward
No need to explain. Just give the answers directly. Thank you.
1. Round off 1.274 to one (1) significant figure
2. Round off 1653 to one (1) significant figure
3. Round off 534.5 to three (3) significant figures
arrow_forward
Please solve the image.
arrow_forward
Please answer all and please do the calculations
arrow_forward
part A: Sort the following numbers according to whether they should be rounded up or down when rounding to the nearest tenth (the first digit after the decimal).
3.1760, 4.319, 19.47, 5.82, 66.9214, 8878.2010, 7.084, 124.76
part B: Drag the answers that have been correctly rounded to the appropriate number of significant figures to their place in the table. To avoid rounding errors, start with the unrounded value before conducting each manipulation.
Drag the appropriate labels to their respective targets.
View Available Hint(s)for Part B
Reset
Help
14.93
Group 3 14.93
12
Group 1 12
14.92
Group 3 14.92
3.62
Group 4 3.62
14
Group 3 14
3.7
Group 4 3.7
15
Group 3 15
3.6
Group 4 3.6
15.0
Group 3 15.0
3.63
Group 4 3.63
14.9
Group 3 14.9
3.623
Group 4 3.623
12.47
Group 1 12.47
7.97
Group 2 7.97
12.46
Group 1 12.46
7.966
Group 2 7.966
12.4
Group 1 12.4
7.0
Group 2 7.0
13
Group 1 13
7.96
Group 2 7.96
12.5
Group 1 12.5
8.0
Group 2 8.0
3.622
Group 1…
arrow_forward
Do the indicated arithmetic and give the answer to the correct number of significant figures.
I.
II. 0.71 + 92.2
III. 934 × 0.00435 + 107
IV. (847.89 - 847.73) + 14673
arrow_forward
56. Round the number on the left to the number of significant
figures indicated by the example in the first row. (Use
scientific notation as needed to avoid ambiguity.)
Rounded to 4 Rounded to 2 Rounded to 1
Significant
Figures
Significant
Figures
Significant
Figure
Number
9 × 101
94.52118
94.52
95
105.4545
0.455981
0.009999991
arrow_forward
1. All answers to be entered via short answer are in the NUMERICAL FORMAT and presented up to the 3rd decimal place. ADD TRAILING ZEROS if necessary, to complete your answer. NO NEED TO INCLUDE THE UNIT for now.For uniformity of answers, please be guided by the following examples:- If your answer is 5.627594, enter 5.628- If your answer is 3.129934, enter 3.130- If your answer is 8.38, enter 8.380- If your answer is 1.2, enter 1.200- If your answer is 25, enter 25.000- If your answer is less than the value of 1, always place a zero before the decimal point (E.g.: if 0.5, enter 0.500)2. In cases for answers in the EXPONENTIAL FORMAT, please be guided by the following examples and format:- Do not convert your answer to decimal format- If your answer from the calculator is 1.23454566 x 10E-4, enter 1.235x10^-4 (no spaces in between)- If your answer from the calculator is 7.379566 x 10E-5, enter 7.38x10^-5 (no spaces in between)3. The ATOMIC MASSES should be rounded to the NEAREST WHOLE…
arrow_forward
between significant digits are always significant.
figures.
Example: 5,007 has 4 significant figures.
3) Trailing zeros in a number are significant only If the
number contalns a decimal polnt.
Example: 100.0 has 4 significant figures.
100 has 1 significant figure.
4) Zeros in the beginning of a number whose only function
Is to place the decimal polnt are not significant.
Example: 0.0025 has 2 significant figures.
5) Zeros following a decimal significant figure are
significant.
Example: 0.000470 has 3 significant figures.
0.47000 has 5 signlficant figures.
Determine the number of significant figures in the following numbers.
1. 0.02
6. 5,000.
4.
2. 0.020
2.
7. 6,051.006
3. 501 3
8. 0.0005 1.
4. 501.0
9. 0.1020
5. 5,000
10. 10,001 5
Determine the location of the last significant place value by placing a bar over the digit.
Example: 1.700)
9,010.0
4.7x10-8
10,8 00,000
3.0Tx 1021
0.00410
1. 8040
6. 90,100
0.0300
699.5
2,000X162
0.90100
2. 0.0300
7. 4.7 x 108
3. 699.5
8. 10,800,000.
3.…
arrow_forward
Mass (g)
Height (cm)
Diameter (cm)
Cylinder A
15.560
5.11
1.20
Cylinder B
35.536
5.90
1.30
In your calculation use the value 3.14 for π. Write your answer to the correct number of significant figures.
Calculate the volume of Cylinder A and B using the dimensions of the cylinder.
arrow_forward
part 1
Which of the following is a best practice in weighing solid samples?
Use weighing paper, a watch glass, a beaker, or some other container to measure mass of your solid samples.
Do not return the mass settings to zero mark; let the next user tare it for you.
Place chemicals directly on the balance pan.
For different trials of an experiment, use multiple balances for your measurements
arrow_forward
55. Round the number on the left to the number of significant
figures indicated by the example in the first row. (Use
scientific notation as needed to avoid ambiguity.)
Rounded to
Rounded to
Rounded to
4 Significant 2 Significant 1 Significant
Figures
Number
Figures
Figure
1.45815
1.458
1.5
8.32466
84.57225
132.5512
arrow_forward
g and a glass of water has a mass of 0.050 kg.
An oxygen atom has a mass of 2.66 × 10
Use this information to answer the questions below. Be sure your answers have the correct number of significant digits.
What is the mass of 1 mole of oxygen atoms?
Round your answer to 3 significant digits.
How many moles of oxygen atoms have a mass equal to
the mass of a glass of water?
Round your answer to 2 significant digits.
0
g
x10
X
S
arrow_forward
How many significant figures are in the following measurement:
0.00204 g
Type your answer...
Perform the following calculation. Enter the answer with the correct number of significant figure.
8.934+ 37.1
29
Be sure to start your answer with 0.xxxx, not just a decimal place, if appropriate.
Ex. Enter 0.244 and NOT.244
Type your answer...
Convert 69. kL to uL.
Express your answer in scientific notation without writing units.
Ex. 0.00222 is entered as 2.22*10^-3.
Type your answer...
arrow_forward
I think I did a calculation wrong but I am having trouble understanding significant figures.
In this problem, I am calculation the density of water from my previous calculations mass= 7.359g and volume=7.8mL. So I then divided 7.359g by 7.8mL to find density and got (.9434615385) on my calculator which I then turned into (.94) because I believe there should be 2 significant figures. Is (.94) correct or should 1.4 be the final answer?
arrow_forward
Do the following multiplication and division calculations. Give a final answer with the correct number of significant figures and the correct units. Units can cancel or multiply just like number factors.
(2.5 x 103 m/s) x (5.00 x 10-6 s) = ?
arrow_forward
Please don't provide handwritten solution .....
arrow_forward
Please answer this question as fast as you can please and tahnk you. I will afterwards write an wonderful review on solving the question. Thank you.
Carry out the following calculations, making sure that your answer has the correct number of significant figures.
5.48 x 12.73 = ?
arrow_forward
Do the following calculations to the correct number of significant figures:
MUST follow the rules of SIGNIFICANT figures
a.) 432/7.3-28.523
b.) 0.004 + 0.09879
c.)87.6 + 9.888 +2.3 + 100.77
d.) 5.01 x 105/7.8 x 102
arrow_forward
Answer all
arrow_forward
A sample of gold alloy has a mass of 9.3 kg. It is determined that 0.6 kg of the alloy is actually made up of copper and zinc, with the remainder being gold. Calculate the percentage of this gold in the alloy? Express your answer to the nearest percentage (nearest ones place). Hint: calculate the mass in grams of the gold in the alloy, divide by the whole mass of the alloy, and multiply by 100%. Round your answer to two significant figures.
(I had to alter the wording of this question since it wasn't calculating significant figures properly, so if you got it wrong because of significant figures you can assume you probably actually got it correct.)
arrow_forward
Leaming Goal:
To learn how to round an answer to the correct number of significant
figures.
Multiplication and division
When multiplying or dividing, the final answer is rounded to the same number of significant figures as the measured number with the fewest significant figures.
When we report a measurement in science, we are careful to report only
digits known with certainty, plus a final digit that is recognized to be
uncertain. We call this set of digits significant figures. Often, these numbers
are used in calculations. When we use a calculator, the calculator does not
automatically account for significant figures, so we have to do so ourselves.
There are some basic rules for handling significant figures in calculations as
shown in the table and outlined to the right.
Addition and subtraction
When adding or subtracting, the final answer is rounded to the same number of digits to the right of the decimal point as the measured number with the fewest digits to the right of
the decimal…
arrow_forward
I have a chemistry question, it asks: "In the lab, you measure the density of a metal to be 4.16 g/cm3. The handbook value for the density of this metal is 4.018 g/mL. What is the percent error? Pay close attention to the significant figures in your answer, as you should in the lab."
My question is: What do we do? Are we trying to find the volume and mass from the given density of 4.018? How do we do that?
arrow_forward
what is
x = ?
2. How many significant figures are there in the experimental number:
33.7
arrow_forward
Round each answer to the correct number of significant figures.
9 +2.8 - 0.135+10.8=22.265
My previous answer was 22.3 it was incorrected.
arrow_forward
Five silver coins are added to 454.0 mL of water. The water level rises to a volume of 545.0 mL. What is the volume of the five silver coins? Express your answer with the correct number of significant figures.
Write your final answer in the space below.
Don't forget to show your calculations for your answer at the end of this quiz. Please include the question number with your calculations so I know which question they are for.
arrow_forward
A jet airplane reaches 843. km /h on a certain flight. What distance does it cover in 15.0 min? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also , be sure your answer includes all the correct unit symbols.
arrow_forward
[Review Topics]
[References]
Use the References to access important values if needed for this question.
Write each of the following numbers to 3 significant figures in exponential or scientific notation. Write each number with
only one non-zero digit before the decimal point.
0.000897
6260
0.000903
523000
arrow_forward
SEE MORE QUESTIONS
Recommended textbooks for you
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Related Questions
- 2. Do the following calculations and use the correct number of significant figures in your answers. Assume all numbers are the results of measurements. a. 0.208 + 4.9 + 1.11 b. 228 + 0.999 + 1.02 c. 8.543 − 7.954 d.(3.2 × 10−2) + (5.5 × 10−1) (hint: Write in the decimal form first, then add.) e. 336.86 − 309.11 f. 21.66 − 0.02387arrow_forwardFind the difference between the value of x2 and the sum of x1 plus x3.; let x4 be equivalent to the sum of x1 and x3 and let x5 be the difference between x2 and x5. This calculation scheme is shown below. Make notes about any similarities or differences between the values in your notes. x4 = x1 + x3 x5 = x2 – x4 Data Analyis This section will include all data collected during the lab. Thermochemical Data Tinitial (°C) Tfinal (°C) ΔT (°C) moles NaOH qreaction (kJ) ΔHrxn Reaction 1 25.0 30.3 +5.3 0.025 -1.11 -44.4 Reaction 2 25.0 37.0 +12.0 0.025 -2.51 -100.4 Reaction 3 25.0 31.7 +6.7 0.025 -1.40 -56.1 Reaction 1: NaOH(s) → Na+(aq) + OH-(aq) + x1 kJ 1g /39.977g/mol = 0.025 moles Moles NaOH = 0.025 qsolution = (4.184 J/g °C) (50.0g) (30.3°C -25.0°C) = -1108.76 J/ 1000 qreaction (kJ) = -1.11 kJ ΔH = -1.11 kJ/ 0.025 moles ΔHrxn = -44.4 kJ/mol…arrow_forwardNo need to explain. Just give the answers directly. Thank you. 1. Round off 1.274 to one (1) significant figure 2. Round off 1653 to one (1) significant figure 3. Round off 534.5 to three (3) significant figuresarrow_forward
- Please solve the image.arrow_forwardPlease answer all and please do the calculationsarrow_forwardpart A: Sort the following numbers according to whether they should be rounded up or down when rounding to the nearest tenth (the first digit after the decimal). 3.1760, 4.319, 19.47, 5.82, 66.9214, 8878.2010, 7.084, 124.76 part B: Drag the answers that have been correctly rounded to the appropriate number of significant figures to their place in the table. To avoid rounding errors, start with the unrounded value before conducting each manipulation. Drag the appropriate labels to their respective targets. View Available Hint(s)for Part B Reset Help 14.93 Group 3 14.93 12 Group 1 12 14.92 Group 3 14.92 3.62 Group 4 3.62 14 Group 3 14 3.7 Group 4 3.7 15 Group 3 15 3.6 Group 4 3.6 15.0 Group 3 15.0 3.63 Group 4 3.63 14.9 Group 3 14.9 3.623 Group 4 3.623 12.47 Group 1 12.47 7.97 Group 2 7.97 12.46 Group 1 12.46 7.966 Group 2 7.966 12.4 Group 1 12.4 7.0 Group 2 7.0 13 Group 1 13 7.96 Group 2 7.96 12.5 Group 1 12.5 8.0 Group 2 8.0 3.622 Group 1…arrow_forward
- Do the indicated arithmetic and give the answer to the correct number of significant figures. I. II. 0.71 + 92.2 III. 934 × 0.00435 + 107 IV. (847.89 - 847.73) + 14673arrow_forward56. Round the number on the left to the number of significant figures indicated by the example in the first row. (Use scientific notation as needed to avoid ambiguity.) Rounded to 4 Rounded to 2 Rounded to 1 Significant Figures Significant Figures Significant Figure Number 9 × 101 94.52118 94.52 95 105.4545 0.455981 0.009999991arrow_forward1. All answers to be entered via short answer are in the NUMERICAL FORMAT and presented up to the 3rd decimal place. ADD TRAILING ZEROS if necessary, to complete your answer. NO NEED TO INCLUDE THE UNIT for now.For uniformity of answers, please be guided by the following examples:- If your answer is 5.627594, enter 5.628- If your answer is 3.129934, enter 3.130- If your answer is 8.38, enter 8.380- If your answer is 1.2, enter 1.200- If your answer is 25, enter 25.000- If your answer is less than the value of 1, always place a zero before the decimal point (E.g.: if 0.5, enter 0.500)2. In cases for answers in the EXPONENTIAL FORMAT, please be guided by the following examples and format:- Do not convert your answer to decimal format- If your answer from the calculator is 1.23454566 x 10E-4, enter 1.235x10^-4 (no spaces in between)- If your answer from the calculator is 7.379566 x 10E-5, enter 7.38x10^-5 (no spaces in between)3. The ATOMIC MASSES should be rounded to the NEAREST WHOLE…arrow_forward
- between significant digits are always significant. figures. Example: 5,007 has 4 significant figures. 3) Trailing zeros in a number are significant only If the number contalns a decimal polnt. Example: 100.0 has 4 significant figures. 100 has 1 significant figure. 4) Zeros in the beginning of a number whose only function Is to place the decimal polnt are not significant. Example: 0.0025 has 2 significant figures. 5) Zeros following a decimal significant figure are significant. Example: 0.000470 has 3 significant figures. 0.47000 has 5 signlficant figures. Determine the number of significant figures in the following numbers. 1. 0.02 6. 5,000. 4. 2. 0.020 2. 7. 6,051.006 3. 501 3 8. 0.0005 1. 4. 501.0 9. 0.1020 5. 5,000 10. 10,001 5 Determine the location of the last significant place value by placing a bar over the digit. Example: 1.700) 9,010.0 4.7x10-8 10,8 00,000 3.0Tx 1021 0.00410 1. 8040 6. 90,100 0.0300 699.5 2,000X162 0.90100 2. 0.0300 7. 4.7 x 108 3. 699.5 8. 10,800,000. 3.…arrow_forwardMass (g) Height (cm) Diameter (cm) Cylinder A 15.560 5.11 1.20 Cylinder B 35.536 5.90 1.30 In your calculation use the value 3.14 for π. Write your answer to the correct number of significant figures. Calculate the volume of Cylinder A and B using the dimensions of the cylinder.arrow_forwardpart 1 Which of the following is a best practice in weighing solid samples? Use weighing paper, a watch glass, a beaker, or some other container to measure mass of your solid samples. Do not return the mass settings to zero mark; let the next user tare it for you. Place chemicals directly on the balance pan. For different trials of an experiment, use multiple balances for your measurementsarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning