Copper Cycle Lab Report
docx
keyboard_arrow_up
School
University of Texas *
*We aren’t endorsed by this school
Course
301
Subject
Chemistry
Date
Jun 13, 2024
Type
docx
Pages
12
Uploaded by DrSparrowMaster1191
The Copper Cycle
Samantha Delaunay
Cory Silguero
The University of Texas at Austin
1
P. Sotelo SP2024
Redox reactions stand as prominent methods for producing valuable compounds. In light of increasing awareness of green chemistry, there's been a search for sustainable routes to redox reactions. This has led to significant interest in photoredox catalysis, a burgeoning field where molecules undergo oxidation or reduction using visible light – a vast natural resource. This tutorial paper offers an introductory overview of photoredox catalysis, accompanied by select examples, with the aim of inspiring further exploration and advancement in this rapidly evolving research domain.
In a comprehensive study, researchers investigated the oxygen redox reaction and structural reversibility of NCM or NCA, promising cathode materials for high-energy-density Li-
ion batteries. Utilizing synchrotron X-ray absorption spectroscopy, scanning transmission electron microscopy, and density functional theory calculations, they uncovered that oxygen redox occurs due to cation mixing upon delithiation, despite the absence of Li-O-Li configurations in its pristine form. The formation of the I41 structure was linked to the migration
of transition metals in deeply delithiated material, extending the phase transformation route from layered to rock-salt structure. These findings deepen the understanding of oxygen redox and its impact on structural transformations in Ni-rich layered oxides, offering insights for enhancing cathode material performance in next-generation Li-ion batteries.
Antoine Lavoisier's dedication to precise measurement was evident in his meticulous experiments. In one experiment, burned phosphorus and observed the formation of a white flaky product. Although the phosphorus, the reactant in this case, was not soluble in water, the product was. Therefore, he collected the product, separating it from the unreacted phosphorus through thorough washing with water. After drying, he could measure the amount of phosphorus that had
burned, the quantity of oxygen consumed, and the mass of the resulting product. Through his experiments, he consistently found that the mass of the product equaled the sum of the masses of the consumed reactants. This discovery laid the foundation for the law of conservation of mass.
Examining the Hindenburg disaster of 1937 provides a chemical perspective on oxidation-reduction reactions. The dirigible, filled with hydrogen, utilized this gas to maintain buoyancy. Unfortunately, during its voyage from Germany to the United States, the airship met a
tragic end due to the explosive reaction between hydrogen and oxygen. In this event, hydrogen lost electrons, undergoing oxidation, while oxygen gained electrons, experiencing reduction.
Metallic copper will undergo a sequence of reactions with different reagents to generate four distinct copper compounds, followed by its restoration to its original metallic state. Each reaction's chemical and physical alterations will be observed and documented, with balanced chemical equations being formulated and categorized. The final step involves determining the percent recovery of the initial copper product.
2
P. Sotelo SP2024
Table 1. Initial and final masses of Cu
(s). Description
Mass (g)
Cu
(s)
wire
0.361
Evaporating dish
25.906
Evap. dish + Cu
(s)
product
26.193
Cu
(s)
product
0.287
Table 2.
Observations for Reactions 1-5.
Reaction
Product
Observations
1
Cu(NO
3
)
2
Emits brown gas, turns a blue color 2
Cu(OH)
2
Neon/bright blue, pH paper is blue on first test
3
CuO
Bright blue to dark blue to black cloud
4
CuSO
4
Light blue, burnt Cheeto wire
5
Cu
(s)
Orange copper precipitate, stinky
3
P. Sotelo SP2024
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
For the first step of the copper cycle, copper metal (Cu) reacts with nitric acid (HNO3) to form copper(II) nitrate (Cu(NO3)2). The initial reddish-brown metallic copper turns into a blue solution of copper(II) nitrate. Figure 1:
End of Step 1 Copper Cycle
Next, Copper(II) nitrate (Cu(NO3)2) reacts with sodium hydroxide (NaOH) to form copper(II) hydroxide (Cu(OH)2) A blue solution of copper(II) nitrate reacts with colorless sodium hydroxide to form a blue-green precipitate of copper(II) hydroxide. Figure 2:
End of Step 2 Copper Cycle
4
P. Sotelo SP2024
Thirdly, Copper(II) hydroxide (Cu(OH)2) decomposes upon heating to form copper(II) oxide (CuO). The blue-green liquid of copper(II) hydroxide turns into a black solid of copper(II) oxide with a clear liquid. Figure 3:
End of Step 3 Copper Cycle
After this, Copper(II) oxide (CuO) reacts with sulfuric acid (H2SO4) to form copper(II) sulfate (CuSO4) and water (H2O). The black solid of copper(II) oxide dissolves in the sulfuric acid solution to form a blue solution of copper(II) sulfate. Figure 4:
End of Step 4 Copper Cycle
5
P. Sotelo SP2024
Finally, Copper(II) sulfate (CuSO4) reacts with metallic aluminum (Al) to form metallic copper (Cu). The blue solution of copper(II) sulfate reacts with metallic aluminum to deposit metallic copper onto the aluminum surface and the liquid will become more clear as the copper forms. Figure 5:
End of Step 5 Copper Cycle
The formation of precipitates in some reactions is attributed to the low solubility of certain copper compounds. Insoluble or sparingly soluble compounds tend to precipitate out of solution, whereas soluble compounds remain dissolved.
Step 1 is a redox reaction, step 2 is a precipitation reaction, step three is a decomposition reaction, step 4 is an acid-base reaction, and step 5 is also a redox reaction. Their according chemical equation requirements are described below.
Step 2 Precipitation Reaction:
Balanced Formula Unit:
Cu(NO
3
)
2 (aq) + 2 NaOH
(aq) → Cu(OH)
2 (s) + 2 NaNO
3 (aq)
Total Ionic:
Cu
+2
(aq) + 2 NO
3
-
(aq) + 2 Na
+
(aq) + 2 OH
-
(aq) → Cu(OH)
2 (s) + 2 Na
+
(aq) + 2 NO
3
-
(aq)
Net Ionic:
Cu
2+
(aq) + 2 OH
-
(aq)
→ Cu(OH)
2 (s)
Step 4 Acid-Base Reaction:
Balanced Formula Unit:
CuO
(s)
+ H
2
SO
4 (aq) → CuSO
4 (aq) + H
2
O
(l)
6
P. Sotelo SP2024
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
Total Ionic:
CuO
(s)
+ 2 H
+
(aq) + SO
2-
4 (aq) → Cu
2+ (aq) + SO
2-
4 (aq) + H
2
O
(l)
Net Ionic:
CuO
(s)
+ 2 H
+
(aq) → Cu
2+ (aq) + H
2
O
(l)
Step 3 Decomposition Reaction:
Balanced Chemical Equation:
Cu(OH)
2 (s)
→ CuO
(s) + H
2
O
(1)
Step 1 Redox Reaction:
Balanced Chemical Equation:
Cu
(s)
+ 4 HNO
3 (aq) → Cu(NO
3
)
2 (aq) + 2 NO
2 (g) + 2 H
2
O
(l)
Oxidizing Half Reaction: Cu
(s) → Cu
2+
(aq) + 2e
-
Reduction Half Reaction: 4 H
+
(aq) + 4e
- + 2 NO
3
-
(aq) → 2 NO
2 (g) + 2 H
2
O
(l)
Oxidizing Agent: Nitric Acid (HNO
3
)
Reduction Agent: Copper (Cu)
Step 5 Redox Reaction:
Balanced Chemical Equation:
3 CuSO
4 (aq)
+ 2 Al
(s) → 3 Cu
(s) + Al
2
(SO
4
)
3 (aq)
Oxidizing Half Reaction: 2 Al
(s) → 2 Al
3+
(aq) + 6e
-
Reduction Half Reaction: 3 Cu
2+ (aq) + 6e
- → 3 Cu
(s) Oxidizing Agent: Copper Sulfate (CuSO
4
)
Reduction Agent: Aluminum (Al)
Based on the balanced chemical equation for Reaction 5, the compounds being removed are copper sulfate (CuSO
4
) and aluminum sulfate (Al
2
(SO
4
)
3
). Ethanol has a relatively low boiling point and evaporates quickly at room temperature. By rinsing the copper product with ethanol, residual water from previous washing steps can evaporate more effectively, aiding in drying. Ethanol is generally considered compatible with copper and does not react chemically with it under normal conditions. This ensures that the washing solvent does not introduce any additional contaminants or react with the copper product.
7
P. Sotelo SP2024
A steam bath was the chosen method to dry the copper product because it prevents the oxidation of the copper product by avoiding direct exposure to atmospheric oxygen.
The percent recovery of the copper is 79.5%. The Law of Conservation of Mass is a fundamental principle in chemistry that states that in a chemical reaction, mass is neither created nor destroyed. The total mass of the reactants before a chemical reaction is equal to the total mass of products after the reaction. If the percent recovery is not 100%, it may be caused by an incomplete drying process. If residual water is left behind,
it can lead to an overestimation of its mass during the weighing process. Another reason is the overheating of copper during the drying procedure. This can lead to the oxidation of the product through atmospheric oxygen. Percent Recovery:
(0.287 g / 0.361 g) x 100% = 79.5%
If the percent recovery is above 100%, it may be caused by the contamination of impurities in the final copper recovered which can lead to the overestimation of the final mass.
Another reason is the loss of copper product during the various chemical reactions along the way. If the percent recovery is below 50%, it may be caused by an early completion of step 5. If the copper being recovered on the aluminum wire has not fully formed and was taken out too early, it will be a lower mass than the original copper wire. Another reason is the loss of product during the washing process. 8
P. Sotelo SP2024
REFERENCES 1.
Cauwenbergh, Robin, and Shoubhik Das. “Photocatalysis: A Green Tool for Redox Reactions.”
Synlett
, Georg Thieme Verlag KG, 9 June 2022, www.thieme-connect.com/products/ejournals/abstract/10.1055/s-0040-1706042
.
2.
Li, Shuwei, et al. “Anionic Redox Reaction and Structural Evolution of NI-Rich Layered Oxide Cathode Material.”
Nano Energy
, Elsevier, 4 May 2022, www.sciencedirect.com/science/article/abs/pii/S221128552200413X?via%3Dihub
.
3.
“Lavoisier.”
Chemistry LibreTexts
, Libretexts, 13 June 2023, chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(
Eames)/Chemistry_Basics/Lavoisier.
4.
Web Solutions LLC. “Oxidation-Reduction Reaction - History, Oxidation Numbers, Corrosion, Biological Processes, Current and Future Uses - Examples of Oxidation-
Reduction Reactions.”
History, Oxidation Numbers, Corrosion, Biological Processes, Current And Future Uses - Examples of Oxidation-Reduction Reactions - JRank Articles
, 2023, science.jrank.org/pages/4964/Oxidation-Reduction-Reaction.html.
9
P. Sotelo SP2024
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
10
P. Sotelo SP2024
11
P. Sotelo SP2024
12
P. Sotelo SP2024
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 Documents
Related Questions
The acid-catalyzed hydrolysis of sucrose, C12H22O11 + H₂O + H+ -> C6H12O6 + C6H12O6
+ H+ is known as "inversion of sucrose" because the angle, a, by which the solution
rotates polarized light changes from positive to negative as the reaction proceeds
(data from 30 degree C):
t/hr
a
0
78
2
71
4
12
18
24
42
65.10 44.60 32.40 22.45 2.30
48
-1.96
61
-9
86
95
-15.80 -17.25 -21.15
∞
Use this data to show that the reaction is first order and determine its rate coefficient
(at 30 degree C).
arrow_forward
Why does the product (a•b), rather than the sum (a + b) appear in the Law of Mass Action?
This is sometimes brought up to demonstrate how/why nonlinear terms arise in differential equations. The law of mass action states that The rate of a chemical reaction involving an interaction of two or more chemical species is proportional to the product of the concentrations of the given species.
This is NOT an assignment...I'm just curious and trying to understand mathematical relations better. Thanks!
arrow_forward
Thank you in advance for your help!
arrow_forward
За.
Bromine and methanoic acid react in aqueous solution.
Br, (aq) + HCO0Н (ад) — 2Br (aq) + 2H" (аq) + Со, (g)
The reaction was monitored by measuring the volume of carbon dioxide produced as time
progressed.
o 5 10 15 20 25
[Source: © International Baccalaureate Organization 2019]
30
20
40
60
80
100
120
140
160
Time / s
[Source: © International Baccalaureate Organization 2019]
Determine from the graph the rate of reaction at 20 s, in cm³ s1, showing your working.
3b.
Outline, with a reason, another property that could be monitored to measure the rate of this
reaction.
3c.
Describe one systematic error associated with the use of the gas syringe, and how the error
affects the calculated rate.
3d.
Identify one error associated with the use of an accurate stopwatch.
Volume of carbon dioxide / cm
T m mm mo
arrow_forward
What is the Qc value for this equation? Which direction will the reaction shift?
Given: CO(g)+H2O(g)=CO2(g)+H2(g)
Kc = 1.0
• [CO2(g)]= 2.0M
• [H2(g)]= 2.0 M
• [CO(g)]= 1.0 M
• [H2O(g)]= 1.0 M
arrow_forward
hello maam/sir, kindly help me with this numbers please... kindly provide complete solution.. I PROMISE to give 5 star rating directly
arrow_forward
Consider the reaction
a A(aq) → bB(aq)
(1)
Where a and b are stoichiometric coefficients for the balanced chemical reaction The average
reaction rate r can be measured if the concentration change of the reagents or products is
known:
1 ΔΙΑ
1 Δ
r =
and
r =
At
b At
a
where A and B notate the concentration of A and B in solution, and A is always defined
as the difference between "final" and "initial": A[4] = [A],2 - [4],1
and At = t2 – t .
-
A particular case of eq. (1) could be
A(aq) → 2 B(aq)
If the initial concentration of B is 0.2569 mol L1, and after 415.6 s it increases to 0.4633
mol L1, what is the rate of the reaction in mol L1s?
mol L-1 s1. (Use scientific notation)
arrow_forward
The enzyme urease increases the rate of urea hydrolysis at pH 8.0 and 20 °C by a factor of 1014.
Suppose that a given quantity of urease can completely hydrolyze a given quantity of urea in 19 minutes at pH 8.0 and 20 °C.
How long would it take for this amount of urea to be hydrolyzed in the absence of urease at the same temperature and pH in
sterile conditions? Include two significant figures in your answer.
timeuncatalyzed
years
* TOOLS
x10
arrow_forward
Strontium phosphate, Sr3(PO4)2Sr3(PO4)2, dissociates when placed in water. This compound has a solubility of 0.112 mg/L in water at 20 °C.
Calculate the Ksp of Sr3(PO4)2Sr3(PO4)2. Please write your answer using scientific notation according to the following format: 0.0010 would be writen as 1.0*10^-3.
arrow_forward
arrow_forward
-1000
Decomposition Rezctions
Carbon Reduction Reactions
AH
AS
(kJ)
(JK-mol)
O 2 Ag,0(s) → 4 Ag(s) + O2(g)
+62.2
+132.7
O 2 MgO(s) → 2 Mg(s) + O2(g)
+1202.4
+216.7
1000-
O 2 AlhO3(s) → 4 Al(s) – 3 02(g)
+3351.4
+546.8
O 2 Fe2O3(s) → 4 Fe(s) – 3 O2(g)
+1648 4
+5515
O 2 HgO(s) → 2 Hg(t) + 0,(g)
+181.7
+286.8
2000-
O 2 Cr,03(s) → 4 Cr(s)– 3 0,(g)
2269 4
+548.4
Temperature
3000
300
300 K
2000
Temperature ((K)
Clear Graph
The metals Mg and Al, like most metals in groups 1A, 2A, and 3A of the periodic table, cannot be obtained by chemical reduction with carbon at reasonable
temperatures. What procesS Is used to obtain these metals from their ores?
positive
arrow_forward
A time-dependent pressure profile for the reversible reaction between A
and B gases to produce C gas is shown below. The plot is for the reaction being
completed at 375 K. Answer the two questions about this plot.
Give the balanced
Pressure as a Function of Reaction Time
equation in the box provided.
-PA
1.0
Pc
P, atm
PR
B
time
When this same reaction is completed at 475 K, Kp = 5.7.
Does this indicate the reaction has AH > 0 or AH < 0? Explain your choice.
Your answer
arrow_forward
The reaction between peroxodisulphate (VI) ions, S2O8^2- and iodide ions, I- can be catalyzed by iron(III) ions, Fe^3+.a). Suggest a mechanism for the catalytic reaction.
b). Sketch energy profile diagram for the catalyzed and uncatalyzed reactions.
arrow_forward
Reaction 1
FeO(s) + CO(g) → Fe(1) + CO2(g)
AG" > 0
Reaction 2:
C(s) + CO2(g) → 2 CO(g)
AGzn <0
Overall reaction:
FeO(s) + C(s) → Fe(l) + CO(g)
AG n < 0
Subm
The chemical equations above represent the main reactions that occur during the production of Fe(l) under certain conditions. The overall reaction couples reactions 1 and 2, resulting in a
< 0?
thermodynamically favorable process. Which of the following best explains whether or not a particle diagram could represent how the coupling of reaction 1 and reaction 2 results in AG
A particle diagram that represents the increase in the volume of gaseous product particles would be a good representation of how the coupling of reactions 1 and 2 results in a
thermodynamically favorable process.
A particle diagram that represents the decrease in the average kinetic energy of the particles would be a good representation of how the coupling of reactions 1 and 2 results in a
thermodynamically favorable process.
A particle diagram cannot represent…
arrow_forward
Static fatigue depends on a chemical reaction and, as a result, is another example of Arrhenius behavior. Specifically, at a given load, the inverse of time to fracture has been shown to increase exponentially with temperature. The activation energy associated with chemical reaction is 78.6 kJ>mol. If the time to fracture for a soda–lime–silica glass is 1 second at +50°C at a given load, what is the time in hours to fracture at -50°C at the same load?
arrow_forward
21
arrow_forward
Peroxynitric acid (HOONO2) is an unstable molecule that decomposes to nitric acid and oxygen:
2HOONO2(aq) → 2HNO3(aq) + O2(g)When the concentration of peroxynitic acid is graphed against time, the resulting plot is
curved, but if the logarithm of this concentration is plotted, we instead get a straight line.
Based on this, which statement is true?
a) This decay is a second order in peroxynitric acid.
b) The slope of the straight-line graph is the rate constant.
c) One needs the concentration of peroxynitric acid to calculate its half-life.
d) The rate law appears to be of the form -Δ[HOONO2]/Δt = k[HOONO2].
arrow_forward
Use the data given below to find rate constant. Then derive the rate law for this reaction. Show
your work in a separate sheet.
S20g2-(ag) + 31(ag)
2 SO42-(g) +13 (a4)
[S20g2-i (M) [[h (M)
Initial Rate (M/s)
0.30
0.42
4.54
0.44
0.42
6.65
0.44
0.21
3.33
Rate = [36 M -1s-1IS 20 8 2-1]
[86 M -25-1S 20 82-12
Rate =
Rate =
[120 M -25-1S 20 82121]
Rate = [195 M -3s 1S 20 8 21211-2
arrow_forward
1. CzH5OH(I) + HCOOH(I) → HCOOCzHs + H2O(I)
2. C₂H5OH(1)→ C₂H4(g) + H₂O(1)
3. C₂H4(9) + Cl₂(g) → C₂H4C12(1)
4. C6H6(1) + Br2(1)→ C6H5Br(1) + HBr(g)
5. 2C4H10(9) + 130₂(g) → 8CO₂(g) + 10H₂O(1)
6. 2C7H8(1) + 150₂(g) → 14CO(g) + 8H₂O(1)
Match each equation above with its reaction type.
Reaction Type
Addition
Complete combustion
Elimination
Esterification
Incomplete combustion
Substitution
Reaction Number from Above
→
◆
◆
Fill in the blanks to complete the following statement. One method used to differentiate between saturated and unsaturated compounds is to add a few drops of
orange-coloured aqueous bromine to samples of each organic compound. If the compound is
◆ the orange colour will quickly fade.
arrow_forward
A student is preparing a solution of sucrose at a specific concentration. They are doing this by weighing out sucrose on a scale, placing it in a volumetric flask, dissolving it in water, and then diluting it up to the mark on the volumetric flask with water. How would the experimental (actual) molar concentration for C12H22O11 differ from the calculated concentration ( higher, lower, or the same) given the following scenarios? Explain.
arrow_forward
Please answer and show work
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: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Related Questions
- The acid-catalyzed hydrolysis of sucrose, C12H22O11 + H₂O + H+ -> C6H12O6 + C6H12O6 + H+ is known as "inversion of sucrose" because the angle, a, by which the solution rotates polarized light changes from positive to negative as the reaction proceeds (data from 30 degree C): t/hr a 0 78 2 71 4 12 18 24 42 65.10 44.60 32.40 22.45 2.30 48 -1.96 61 -9 86 95 -15.80 -17.25 -21.15 ∞ Use this data to show that the reaction is first order and determine its rate coefficient (at 30 degree C).arrow_forwardWhy does the product (a•b), rather than the sum (a + b) appear in the Law of Mass Action? This is sometimes brought up to demonstrate how/why nonlinear terms arise in differential equations. The law of mass action states that The rate of a chemical reaction involving an interaction of two or more chemical species is proportional to the product of the concentrations of the given species. This is NOT an assignment...I'm just curious and trying to understand mathematical relations better. Thanks!arrow_forwardThank you in advance for your help!arrow_forward
- За. Bromine and methanoic acid react in aqueous solution. Br, (aq) + HCO0Н (ад) — 2Br (aq) + 2H" (аq) + Со, (g) The reaction was monitored by measuring the volume of carbon dioxide produced as time progressed. o 5 10 15 20 25 [Source: © International Baccalaureate Organization 2019] 30 20 40 60 80 100 120 140 160 Time / s [Source: © International Baccalaureate Organization 2019] Determine from the graph the rate of reaction at 20 s, in cm³ s1, showing your working. 3b. Outline, with a reason, another property that could be monitored to measure the rate of this reaction. 3c. Describe one systematic error associated with the use of the gas syringe, and how the error affects the calculated rate. 3d. Identify one error associated with the use of an accurate stopwatch. Volume of carbon dioxide / cm T m mm moarrow_forwardWhat is the Qc value for this equation? Which direction will the reaction shift? Given: CO(g)+H2O(g)=CO2(g)+H2(g) Kc = 1.0 • [CO2(g)]= 2.0M • [H2(g)]= 2.0 M • [CO(g)]= 1.0 M • [H2O(g)]= 1.0 Marrow_forwardhello maam/sir, kindly help me with this numbers please... kindly provide complete solution.. I PROMISE to give 5 star rating directlyarrow_forward
- Consider the reaction a A(aq) → bB(aq) (1) Where a and b are stoichiometric coefficients for the balanced chemical reaction The average reaction rate r can be measured if the concentration change of the reagents or products is known: 1 ΔΙΑ 1 Δ r = and r = At b At a where A and B notate the concentration of A and B in solution, and A is always defined as the difference between "final" and "initial": A[4] = [A],2 - [4],1 and At = t2 – t . - A particular case of eq. (1) could be A(aq) → 2 B(aq) If the initial concentration of B is 0.2569 mol L1, and after 415.6 s it increases to 0.4633 mol L1, what is the rate of the reaction in mol L1s? mol L-1 s1. (Use scientific notation)arrow_forwardThe enzyme urease increases the rate of urea hydrolysis at pH 8.0 and 20 °C by a factor of 1014. Suppose that a given quantity of urease can completely hydrolyze a given quantity of urea in 19 minutes at pH 8.0 and 20 °C. How long would it take for this amount of urea to be hydrolyzed in the absence of urease at the same temperature and pH in sterile conditions? Include two significant figures in your answer. timeuncatalyzed years * TOOLS x10arrow_forwardStrontium phosphate, Sr3(PO4)2Sr3(PO4)2, dissociates when placed in water. This compound has a solubility of 0.112 mg/L in water at 20 °C. Calculate the Ksp of Sr3(PO4)2Sr3(PO4)2. Please write your answer using scientific notation according to the following format: 0.0010 would be writen as 1.0*10^-3.arrow_forward
- arrow_forward-1000 Decomposition Rezctions Carbon Reduction Reactions AH AS (kJ) (JK-mol) O 2 Ag,0(s) → 4 Ag(s) + O2(g) +62.2 +132.7 O 2 MgO(s) → 2 Mg(s) + O2(g) +1202.4 +216.7 1000- O 2 AlhO3(s) → 4 Al(s) – 3 02(g) +3351.4 +546.8 O 2 Fe2O3(s) → 4 Fe(s) – 3 O2(g) +1648 4 +5515 O 2 HgO(s) → 2 Hg(t) + 0,(g) +181.7 +286.8 2000- O 2 Cr,03(s) → 4 Cr(s)– 3 0,(g) 2269 4 +548.4 Temperature 3000 300 300 K 2000 Temperature ((K) Clear Graph The metals Mg and Al, like most metals in groups 1A, 2A, and 3A of the periodic table, cannot be obtained by chemical reduction with carbon at reasonable temperatures. What procesS Is used to obtain these metals from their ores? positivearrow_forwardA time-dependent pressure profile for the reversible reaction between A and B gases to produce C gas is shown below. The plot is for the reaction being completed at 375 K. Answer the two questions about this plot. Give the balanced Pressure as a Function of Reaction Time equation in the box provided. -PA 1.0 Pc P, atm PR B time When this same reaction is completed at 475 K, Kp = 5.7. Does this indicate the reaction has AH > 0 or AH < 0? Explain your choice. Your answerarrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_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
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher: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: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning