Alum_F23_V18
pdf
keyboard_arrow_up
School
University of Notre Dame *
*We aren’t endorsed by this school
Course
INORGANIC
Subject
Chemistry
Date
Dec 6, 2023
Type
Pages
8
Uploaded by keira123mendoza
Fall 2023
1
Recrystallizing Alum can take time. Store your recrystallization flask on a tray in lab (see TA). You can take
pictures for your lab report, during make up labs (11/27-12/1); no need an appointment; just go to room 229
anytime the week of M-F 2-4 or W, F 10-12. Example crystals will also be available, if your crystals don’t form.
Synthesis of Alum
Introduction
Aluminum cans are often recycled to make more aluminum products. In this
experiment, you will synthesize a compound called
alum
, starting from the
aluminum in soda cans. The name
alum
refers to a class of chemical compounds
that are valuable for water purification, making explosives, tanning processes,
deodorant sticks, medical astringents, and as shown here, crisping pickles.
What you have learned so far about analogical reasoning and how to construct a
strong scientific argument based on evidence, reasoning and claims are directly transferrable to this
lab. Thus, as you synthesize alum, try to use analogical reasoning and modeling to help you think
about what is happening at the atomic scale. In addition, as you make chemical observations in lab,
think about the evidence you are gathering that will help you make claims and construct a scientific
argument. Your lab report will include the overall yield of the reaction, a discussion about the
observations made in lab, and a hypothesis about how the reaction conditions in each step of the
synthesis of alum changes the chemical state of the aluminum atoms.
Your lab report will be due the day following your next lab session (week of 11/27-12/1).
Since recrystallization can take some time, please see your TA for instructions about including the
results of recrystallization. See section 11. recrystallization, for the reasons behind this
instruction.
In this experiment, you will produce alum from an aluminum can in a multi-step synthesis reaction
summarized by the chemical equation below:
The name “alum” actually describes several related compounds. The compound that you will
synthesize today is potassium aluminum sulfate dodecahydrate [KAl(SO
4
)
2
•
12 H
2
O]. Alum is a type
Goals:
1.
To synthesize alum from aluminum soda cans.
2.
To make observations about each intermediate chemical reaction in the synthesis and to
describe what is happening on the atomic scale.
3.
To calculate the theoretical yield and percent yield of the synthesis reaction.
4.
To construct a discussion about how the interactions of aluminum with other atoms and
molecules changes throughout the synthesis of alum.
5.
To think about the chemical transformations that occur at the atomic scale.
Fall 2023
2
Recrystallizing Alum can take time. Store your recrystallization flask on a tray in lab (see TA). You can take
pictures for your lab report, during make up labs (11/27-12/1); no need an appointment; just go to room 229
anytime the week of M-F 2-4 or W, F 10-12. Example crystals will also be available, if your crystals don’t form.
of compound called a
double salt
because there are two different cations (K
+
and Al
3+
) that
crystallize
together in a single solid. The dot and the 12 H
2
O molecules in the formula signal that the
compound is “hydrated”. These water molecules are included in the unit formula and contribute to
the mass of a single molecule of the compound. Therefore, the molecular weight of potassium
aluminum sulfate dodecahydrate is 474.37 grams/mole.
A.
B.
Figure 1
. Crystal structure of [KAl(SO
4
)
2
•
12H
2
O]. (K = purple, Al = gray, S = yellow, O = red,
H = white). A. KAl(SO
4
)
2
12
•
H
2
O. B. The packing of [KAl(SO
4
)
2
•
12H
2
O] in a crystal.
[Source:
Cambridge Structural Database (file: EVUWAV) accessed 10/2016.
Percent yield and theoretical yield:
Knowing the molar ratios provided by a balanced chemical equation, you can predict the
amount of product (in this case, the amount of alum [KAl(SO
4
)
2
•
12H
2
O] you will produce based on
the amount of each reactant used. This is called the
theoretical yield
. In this synthesis, the
reactants (potassium hydroxide and sulfuric acid) will be used in excess of the molar ratio needed to
complete the reaction.
That means that the limiting reactant will be the amount of aluminum metal
that you start with.
In a synthesis reaction it is difficult to obtain the mass of product predicted by a calculation of
the theoretical yield. There are a number of possible obstacles. Because this is a multi-step reaction,
several intermediate products are formed along the way, each containing aluminum. Different steps
require transfers of the reaction between different glassware, filtration, stirring, etc., all of which
can lead to the loss of some of the intermediate compounds necessary for forming the final alum
product. Therefore, it is useful to calculate the percent yield which provides a comparison of the
actual yield and the theoretical yield:
Fall 2023
3
Recrystallizing Alum can take time. Store your recrystallization flask on a tray in lab (see TA). You can take
pictures for your lab report, during make up labs (11/27-12/1); no need an appointment; just go to room 229
anytime the week of M-F 2-4 or W, F 10-12. Example crystals will also be available, if your crystals don’t form.
Pre-lab Assignment
In your lab notebook, write answers for questions 1-5 below. You must complete the pre-lab before
coming to the lab meeting or you will not be permitted to go into the laboratory.
1.
Write a two to three sentence introduction to the lab.
2.
Figure 1 on page 2 shows a model (i.e. a type of analogy) of the arrangement of atoms in
the solid state structure of alum [KAl(SO
4
)
2
•
12H
2
O]. For example, you can see that the
purple spheres representing potassium ions (K
+
) are surrounded by 6 water molecules.
Since alum is a salt (also called an electrolyte) it is soluble in water. When the solid
dissolves in water, the cations and anions are “solvated” by water. Solvation helps to
stabilize the ions in solution and prevents the cations and anions from recombining.
Although water is neutral, there is a slight negative charge on the oxygen and a slight
positive charge on each hydrogen (see picture here).
d-
Draw a picture to represent the solvation of cations (Al
3+
and K
+
) and anions
O
(SO
4
2-
) when alum dissolves in water.
H
H
d
+
d
+
3.
Create a safety information table that includes the chemicals used in the lab, the
hazards associated with them, and any safety handling precautions.
4.
What volume of 1.5M potassium hydroxide (KOH) solution is needed to react with 1.0
g of aluminum (Al) according to the balanced chemical equation on page 1? (See the
sample “worked problem” below.)
5.
What volume of potassium hydroxide should be used to react with 1.0 g of aluminum if
you want a two-fold molar excess of potassium hydroxide?
Worked Problem:
Starting with approximately 1 g of iron, how much of a 1.55M solution of H
2
SO
4
would
be needed to react according to the equation?
Fe(
s
) + H
2
SO
4
(
aq
)
è
FeSO
4
(
aq
) + H
2
(g)
Step 1. The piece of iron weighed exactly 1.060g. Therefore:
(1.060g Fe) (1.00 mole Fe / 55.845g Fe) = 0.0190 moles Fe
Step 2. According to the balanced equation for the reaction, for every 1 mole of Fe, we need 1 mole of
H
2
SO
4
. Therefore:
we would need 0.0190 moles of H
2
SO
4
.
Step 3. The volume of 1.55M H
2
SO
4
solution required can be calculated:
(0.0190 moles H2SO4) (L/1.55 moles) (1000 mL/ L) = 12.2 mL
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
Fall 2023
4
Recrystallizing Alum can take time. Store your recrystallization flask on a tray in lab (see TA). You can take
pictures for your lab report, during make up labs (11/27-12/1); no need an appointment; just go to room 229
anytime the week of M-F 2-4 or W, F 10-12. Example crystals will also be available, if your crystals don’t form.
There are a variety of ways to answer this question. In all cases, your argument needs to be sufficiently
supported with evidence you gather throughout the experiment. Be sure to carefully observe and
record all steps of the synthesis and pay special attention to the questions as you work through the
procedure.
Laboratory Guide
Please pair up with another student when doing lab work. If there is an odd number of participants
in lab, one group may be permitted to have three people. Record all your observations in your own
lab notebook.
Your lab work will also involve working in partnership on certain activities, answering questions,
discussing observations, or analyzing results. As you go through the experimental guide, you will
notice there are questions that are set off in the guide (i.e. “
Q:
”). For example:
Q:
Companies apply a polymer coating to the inside of the aluminum soda can. Can you guess why?
You are required to respond to these questions in your lab notebook.
Our expectation is that you
write enough to give an indication of what you were thinking about. You do not have to write down
the question AND answer, but you must address the answer, for example: “polymer coating on the
inside is probably for …..”
Goggles are required at all times in the lab.
There are no exceptions. Gloves are available. If you
have questions about safety, please do not hesitate to ask your laboratory instructor. This lab has
portions of the procedure that must be completed under the hood.
Chemicals:
Materials:
aluminum from soda can
Supplies and Equipment*:
1.5 M potassium hydroxide (KOH)
electronic balance
9.0 M sulfuric acid (H
2
SO
4
)
steel wool
ice
glass gravity filtration funnel
50%:50% ethanol:water mixture
gravity filtration filter paper (11 or 12.5 cm
qualitative)
Bunsen burner and ring stand
Buchner funnel and vacuum flask
Buchner funnel filter paper (9.0 cm)
Various glassware, including large beaker for ice
bath
(*illustrations of how to set up filtration equipment are provided in procedure)
Scientific Question:
How do changes in chemical state (solid to solute to crystal) affect the way
aluminum interacts with other chemicals?
•
It can be helpful to include the observations about the reactants, products and relative rates of
the different steps in the alum synthesis and drawings of aluminum at the atomic scale.
Fall 2023
5
Recrystallizing Alum can take time. Store your recrystallization flask on a tray in lab (see TA). You can take
pictures for your lab report, during make up labs (11/27-12/1); no need an appointment; just go to room 229
anytime the week of M-F 2-4 or W, F 10-12. Example crystals will also be available, if your crystals don’t form.
Laboratory Procedure
1.
Obtain a strip of aluminum from a soda can. Using steel wool, scrub both sides of the strip to
remove the paint from the outside and the polymer coating from the inside.
Q:
Companies apply a polymer coating to the inside of the aluminum
soda can. Can you guess why?
2.
Use scissors to cut the strip into tiny pieces and weigh out about 0.7 g of the
metal. It is not important to have exactly 0.700 g of aluminum, but it is
important to record the
exact
mass to ±0.001 g in your lab notebook.
3.
Using your actual mass of aluminum and the concentration of KOH, calculate
the volume of KOH needed to add a two-fold molar excess to the aluminum.
(You should not have to add more than 65 mL of KOH. If your calculation result
is >65 mL, see your lab instructor.)
4.
Place the aluminum pieces in a 250 mL beaker and SLOWLY add the two-fold molar excess of
KOH solution. DO NOT use an Erlenmeyer flask.
Q:
What evidence do you have that a gas is being produced during the reaction?
5.
When the initial bubbling and foaming has slowed, heat the
solution over a Bunsen burner very gently. DO NOT BOIL. If the level
of the liquid drops to less than one quarter of the original level, add
some distilled water. After the fizzing has completely ceased (10-15
minutes) and you no longer see chunks of aluminum in the solution,
remove the beaker from the flame.
Q:
Why can you no longer see the aluminum once the reaction is
complete?
6.
While the solution is still hot, filter it by gravity filtration (see picture
at right for setup), to remove black insoluble impurities. Discard filter
paper and save the filtrate collected in the beaker.
7.
Cool the solution to room temperature and then slowly add 15 mL of 9 M H
2
SO
4
. Stir the
mixture continuously. Record your observations.
Q:
After the reaction occurs, what is the chemical formula of the solid you are observing? What
chemical species are present in the solution?
Fall 2023
6
Recrystallizing Alum can take time. Store your recrystallization flask on a tray in lab (see TA). You can take
pictures for your lab report, during make up labs (11/27-12/1); no need an appointment; just go to room 229
anytime the week of M-F 2-4 or W, F 10-12. Example crystals will also be available, if your crystals don’t form.
8.
Using a Bunsen burner, heat the mixture gently for 10 minutes. Watch carefully for splattering.
The solution should become clear. If any solid is seen, filter the warm mixture again. Record
your observations in your lab notebook.
9.
Cool the resulting clear solution in an ice bath until crystals of alum form. Also, place a small
Erlenmeyer flask containing 20 mL of 50% ethanol/water solution into the ice bath to cool for use in
step 10.
If no crystals form after 15 - 20 minutes, try scratching the inside of the beaker with a glass stirring
rod. The scratching forms small grooves in the glass, and the crystals can adhere to the rough
surface. If you are still unsuccessful in obtaining crystals, boil the solution to reduce the volume of
liquid by 25% and then cool in the ice bath. When crystals begin to form, leave the beaker in ice for
another 10 minutes.
Q:
In reactions a, b, and c, were there any potential ways to lose reactants that are
necessary for the final reaction (step d) to form alum?
10.
Place a circular filter paper into your Buchner funnel (see
setup here). Using vacuum suction, filter and wash the crystals
using
ice cold
ethanol/water solution. It's important that the
ethanol/water solution is very cold. Continue to apply the
vacuum until the filter paper is dry and the crystals do not stick to
a stirring rod if touched
.
Carefully remove the filter paper from the funnel. Select a
clean, empty beaker and weigh it, recording the mass in your
lab notebook. Then transfer the crystals into the beaker by
scraping them from the paper and record the mass of the
beaker plus crystals. Record this in your lab notebook. This is
the mass you will use for determining percent yield. [Note:
your TA may have additional ideas about drying and
transferring the crystals].
Post Lab Question
:
Please note that there is a post lab question that is part of the lab report (see
rubric, “Post Lab Question”). Include the answer to this post lab question right after your analysis, under
a separate heading: What is the percent yield of your synthesis of alum?
(
Provide a brief explanation of
your results).
If you can’t determine the mass of your product (which can sometimes be difficult to do
for a variety of reasons), instead of calculating a percent yield, assume a 90% yield, and provide a
calculation of what mass you would have expected based on a 90% yield.
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
Fall 2023
7
Recrystallizing Alum can take time. Store your recrystallization flask on a tray in lab (see TA). You can take
pictures for your lab report, during make up labs (11/27-12/1); no need an appointment; just go to room 229
anytime the week of M-F 2-4 or W, F 10-12. Example crystals will also be available, if your crystals don’t form.
11.
Recrystallization.
The next step is to recrystallize the alum. Recrystallization is a common
technique for purifying substances. It can increase purity of the solid because impurities are left in
solution. Large crystals often indicate high purity as shown here.
Crystal of alum (source:
https://en.wikipedia.org/wiki/Alum
, accessed Oct 20
23
).
Since recrystallization will take time, you will try to grow your crystals on a tray in lab. Your TA will
show you where this is in lab. Make sure you label the flask with your name. The recrystallization
process will occur over the next week. The instructions are shown below.
Your recrystallization results
do not have to be included in your lab report. However, if you find that you grew nice crystals and
would like to include a picture in your lab report, take a picture with your cell phone (or ask
someone else to take a picture for you) and include it in your report.
For this reason, your lab report
will be due the next day after you inspect your crystals from 11/27-12/1. After you place your samples
for recrystallization on your benchtop, they will be collected by the lab manager. Make sure you label
the flask with your name. You may then go to her office (229 Aubert) anytime M-F 2-4pm or W,F
10am-12 during the week of 11/27-12/1 to view/take pictures of your crystals. If you have questions,
please contact sarah.e.bernard@maine.edu
Recrystallization Procedure:
Transfer approximately 5 g of your alum into a 150 mL beaker, add
30 mL distilled water and heat with stirring to dissolve the solid. When all of the alum has dissolved,
remove the solution from the heat. Carefully place the solution uncovered in your drawer and allow it
to stand until the next laboratory period.
Your TA will advise you of opportunities to include the results of your recrystallization in your lab report.
Fall 2023
8
Recrystallizing Alum can take time. Store your recrystallization flask on a tray in lab (see TA). You can take
pictures for your lab report, during make up labs (11/27-12/1); no need an appointment; just go to room 229
anytime the week of M-F 2-4 or W, F 10-12. Example crystals will also be available, if your crystals don’t form.
Rubric for laboratory reports
(due the week of 11/27-12/1)
Introduction:
(5 pts)
Goal:
To provide a short introduction.
Content:
The summary presents the title of your report, the date the lab work was
done, your partner(s) and a couple of overview sentences about what the lab
experiment was about.
Data, Results,
Evidence:
Scientific data
that supports the
claim.
(25 pts total)
Goal:
To describe what you did and what data was collected and observed.
Downloaded Procedure:
Reference the laboratory procedure that was
downloaded and the date it was accessed (Synthesis of Alum, InterChemNet,
accessed: 10/1/2018). Any changes in procedure should be noted.
Data, Results, and Evidence:
Carefully organize and present the data you collected
and any calculations you performed. We recommend that you include chemical
equations and explanations that are provided to give some insight into what
happens on the atomic scale.
Analysis of
Evidence
(Reasoning)
:
Scientific
explanations that
use evidence to
construct claims.
(30 pts total)
Goal:
To provide the logic to evaluate your data and observations.
Discussion:
Analyze the evidence you will be using to support your claim. It may be
helpful to include a discussion of the underlying chemical transformations as part
of your evidence at both the molecular and macroscopic scales. Hint: Using your
observations in lab and drawings of models representing molecular structure,
discuss the interactions of aluminum with other atoms and molecules; including
aluminum surrounded by other aluminum atoms, surrounded by solvent
molecules, and surrounded by water, potassium and sulfate ions as an alum salt.
Scientific Question:
How do changes in chemical state (solid to solute to crystal) affect the way
aluminum interacts with other chemicals?
Helpful to include observations about reactions and drawings of aluminum at the
atomic scale.
Post Lab
Question
(5 pts)
Include the answer to this post lab question right after your analysis, under a
separate heading:
What is the percent yield of your synthesis of alum?
(
Provide a brief
explanation of your results). If you can’t determine the mass of your product
(which can sometimes be difficult to do for a variety of reasons), instead of
calculating a percent yield, assume a 90% yield, and provide a calculation of
how what mass you would have expected based on a 90% yield.
Claims(s):
Statement(s),
derived from
evidence, using
scientific
reasoning
(15 pts total)
Goal:
To describe what claims or conclusions can be made.
Claims:
Clearly state what claims or conclusions you can make. The logic of your
claims builds from the evidence and reasoning presented in the previous sections.
Please write your claims clearly in order for them to be assessed reasonably.
Related Documents
Related Questions
We have talked about in lecture about metamorphic grade, and about the difference between progradeand retrograde mineral reactions. One such possible mineral reaction is as follows:orthoclase + sillimanite + H2O = muscovite + quartz
3a: Write a balanced chemical reaction for the above minerals, given that the formula for muscovite isK2Al6Si6O20(OH)4
3b: Indicate which reaction direction (left to right, right to left) is the prograde direction, and explainwhy you think that.
arrow_forward
15. Give the product side of the balanced chemical reaction for the following
reaction:
Mg (s) + O2 (g) →
(Caution, check phases!)
Select one:
a. 2 Mgo (s)
b. 3 MgCl2 (aq) + 2 Fe (s)
с. МgO (s)
d. Mg3 (PO4)2 (s) + 3 H20 (1) + 3 CO2 (g)
e. Mg3(PO4)2 (aq) + 3 H20 (1) + 3 CO2 (g)
f. MgCl2 (aq) + Fe (s)
g. MgPO4 (aq) + H2CO3 (aq)
h. MgO (s) + CO2 (g)
i. none of these
j. Mg3 (PO4)2 (aq) + H20 (I) + CO2 (g)
arrow_forward
Period 6 Colleg
bl
When a solution of potassium
chromate, K,Cro, (aq) is added to a
solution of silver nitrate, AGNO,
(aq), a clear solution and an
orange-brown solid are formed.
Could the solid formed be solid
copper, Cu (s)? Explain why or why
not.
Pear DeckNactive Sler
Slide 13/21
arrow_forward
answer the chemistry problem in the image and show solution step by step
arrow_forward
Supply coeffcients that balence the atoms and ions.
Supply electrons (e-) that balence the charges.
Balence the half-equation
1. Pb^2+ -> Pb^4+ ........
2. ....... + Cl2 -> .......... Cl^-
Blanence the following equation
3. ....... ClO3^- -> ........ Cl^- + ........ O2
4. ........ Al +........ Fe^2+ -> ......... Al^3+ + ........ Fe
arrow_forward
INSTRUCTIONS
a. Determine the most probable products from the given reactants based on the indicated
reaction type. Write NO REACTION if the reaction will not proceed based on the given
reactants.
b. IF THE REACTION PROCEEDS: Balance the equation.
c. IF THE REACTION PROCEEDS: Assign the oxidation numbers for all atoms in the
equation and indicate whether it is a redox reaction or not.
d. FOR REDOX REACTIONS: Identify the reduction and oxidation half-reactions, as well as
the reducing and oxidizing agents.
arrow_forward
Read the entire procedure and the recommended safety precautions. you think extra pieces of calcium or magnesium metal should be disposed of down the drain? or why not?
arrow_forward
What mass of carbon dioxide is formed from burning one gallon of octane, C8H18? Octane has a density of 703 kg/m3.1 L = 0.2642 gal 1 lb = 453.592 gAn average tree absorbs 48 pounds of CO2 in one year. How many trees would you need to plant to offset the CO2produced from burning one gallon of octane every day for one year (365 days)?
arrow_forward
1. Copper is found as the mineral covellite (CuS). The first step in extracting the copper is to dissolve
the mineral in nitric acid (HNO3), which oxidizes sulfide to sufate and reduces nitric acid to NO:
CuS) + HNO3(aq)
→ NO(g) + CuSO4
->
Balance this equation using the half- reaction method CHEM
GINEE
RST YEAR
FRANE
6 hra
arrow_forward
Please give information about these chemicals.
arrow_forward
15. Balance the following chemical equations, and identify the reaction type of each
Balanced equation:
Reaction type:
HgO +
F2 -
HØF2 +
O2
КОН +
MgCl2 -
КСІ +
Mg(OH)2
H3PO4 +
Fe(ОН)2 —
H2O +
Fe3(PO4)2
NaCIO3 -
NaCl +
O2
arrow_forward
For all of the following experiments, under standard conditions, which species could be spontaneously produced?
(a) A lead wire is placed in a solution containing Cu2+
No reaction. YES or NO
Cu. YES or NO
PbO2. YES or NO
(b) Crystals of I2 are added to a solution of NaCl.
No reaction. YES or NO
I^-. YES or NO
Na. YES or NO
(c) Cl2 gas is bubbled into a solution of NaI.
Cl^-. YES or NO
No reaction. YES or NO
Na. YES or NO
arrow_forward
STOICHIOMETRY: Please answer only number 81 in the image provided below.
arrow_forward
SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Related Questions
- We have talked about in lecture about metamorphic grade, and about the difference between progradeand retrograde mineral reactions. One such possible mineral reaction is as follows:orthoclase + sillimanite + H2O = muscovite + quartz 3a: Write a balanced chemical reaction for the above minerals, given that the formula for muscovite isK2Al6Si6O20(OH)4 3b: Indicate which reaction direction (left to right, right to left) is the prograde direction, and explainwhy you think that.arrow_forward15. Give the product side of the balanced chemical reaction for the following reaction: Mg (s) + O2 (g) → (Caution, check phases!) Select one: a. 2 Mgo (s) b. 3 MgCl2 (aq) + 2 Fe (s) с. МgO (s) d. Mg3 (PO4)2 (s) + 3 H20 (1) + 3 CO2 (g) e. Mg3(PO4)2 (aq) + 3 H20 (1) + 3 CO2 (g) f. MgCl2 (aq) + Fe (s) g. MgPO4 (aq) + H2CO3 (aq) h. MgO (s) + CO2 (g) i. none of these j. Mg3 (PO4)2 (aq) + H20 (I) + CO2 (g)arrow_forwardPeriod 6 Colleg bl When a solution of potassium chromate, K,Cro, (aq) is added to a solution of silver nitrate, AGNO, (aq), a clear solution and an orange-brown solid are formed. Could the solid formed be solid copper, Cu (s)? Explain why or why not. Pear DeckNactive Sler Slide 13/21arrow_forward
- answer the chemistry problem in the image and show solution step by steparrow_forwardSupply coeffcients that balence the atoms and ions. Supply electrons (e-) that balence the charges. Balence the half-equation 1. Pb^2+ -> Pb^4+ ........ 2. ....... + Cl2 -> .......... Cl^- Blanence the following equation 3. ....... ClO3^- -> ........ Cl^- + ........ O2 4. ........ Al +........ Fe^2+ -> ......... Al^3+ + ........ Fearrow_forwardINSTRUCTIONS a. Determine the most probable products from the given reactants based on the indicated reaction type. Write NO REACTION if the reaction will not proceed based on the given reactants. b. IF THE REACTION PROCEEDS: Balance the equation. c. IF THE REACTION PROCEEDS: Assign the oxidation numbers for all atoms in the equation and indicate whether it is a redox reaction or not. d. FOR REDOX REACTIONS: Identify the reduction and oxidation half-reactions, as well as the reducing and oxidizing agents.arrow_forward
- Read the entire procedure and the recommended safety precautions. you think extra pieces of calcium or magnesium metal should be disposed of down the drain? or why not?arrow_forwardWhat mass of carbon dioxide is formed from burning one gallon of octane, C8H18? Octane has a density of 703 kg/m3.1 L = 0.2642 gal 1 lb = 453.592 gAn average tree absorbs 48 pounds of CO2 in one year. How many trees would you need to plant to offset the CO2produced from burning one gallon of octane every day for one year (365 days)?arrow_forward1. Copper is found as the mineral covellite (CuS). The first step in extracting the copper is to dissolve the mineral in nitric acid (HNO3), which oxidizes sulfide to sufate and reduces nitric acid to NO: CuS) + HNO3(aq) → NO(g) + CuSO4 -> Balance this equation using the half- reaction method CHEM GINEE RST YEAR FRANE 6 hraarrow_forward
- Please give information about these chemicals.arrow_forward15. Balance the following chemical equations, and identify the reaction type of each Balanced equation: Reaction type: HgO + F2 - HØF2 + O2 КОН + MgCl2 - КСІ + Mg(OH)2 H3PO4 + Fe(ОН)2 — H2O + Fe3(PO4)2 NaCIO3 - NaCl + O2arrow_forwardFor all of the following experiments, under standard conditions, which species could be spontaneously produced? (a) A lead wire is placed in a solution containing Cu2+ No reaction. YES or NO Cu. YES or NO PbO2. YES or NO (b) Crystals of I2 are added to a solution of NaCl. No reaction. YES or NO I^-. YES or NO Na. YES or NO (c) Cl2 gas is bubbled into a solution of NaI. Cl^-. YES or NO No reaction. YES or NO Na. YES or NOarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning