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Chemistry
Date
May 4, 2024
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4
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MODULE 7: LESSON 1 ASSIGNMENT CHEM 20 (?/34 MARKS)
Lesson 1 Assignment: Limiting Reagents Lab: Chemical Analysis Using a Graph Read “Lab Exercise 8.A: Chemical Analysis Using a Graph” on page 317 in your textbook. You may also find the information about this reaction on page 318 useful in completing your analysis. After you have read the lab, answer the following questions to complete your analysis. Analysis (2 marks) 1. Write the balanced chemical equation for the reaction described in this lab exercise. Answer: Pb(NO
3
)
2
(aq) + 2KI(aq) -> PbI
2
(s) + 2KNO
3
(aq) (1 mark) 2. Identify the limiting reagent and the excess reagent in this lab. Answer: Limiting Reagent = potassium iodide Excess Reagent = lead (II) nitrate (2 marks) 3. What is observed when the two reacting solutions are mixed? Describe a test that could be performed to ensure that the reactions performed were complete. Answer: - When the two reacting solutions, lead (II) nitrate and potassium iodide are mixed then a bright yellow precipitate is formed. To ensure that the reactions performed were complete them add more of the limiting reagent (potassium iodide) using a medicine dropper into the solution. If any there is still cloudiness that means that the reaction isn’t yet complete. So, continue to add more drops of the limiting reagent (potassium iodide) until no more precipitate forms, because at that point the reaction is complete. 4. Use a spreadsheet to create a graph of the data shown in “
Table 1.
”
In this lab, the manipulated variable is the mass of Pb(NO
3
)
2
reacting. Use your completed graph to answer questions 4.a. and 4.b. (1 mark) a. A lab technician weighs out 2.5 g of Pb(NO
3
)
2
(s) and dissolves it in water. What mass of PbI
2
(s) can be produced from this solution? Answer: Pb(NO
3
)
2
(aq) + 2KI(aq) → 2KNO
3
(aq) + PbI
2
(s) 2.5 g. m ? 331.2 g/mol 461.01 g/mol n[Pb(NO
3
)
2
] = (2.5 g) / (331.2 g/mol) n= 0.00754830917 mol
n(PbI
2
)= (0.00754830917 mol)(1) n= 0.00754830917 mol m(PbI
2
)= (0.00754830917 mol)(461.01 g/mol) m= 3.48 g of PbI
2 can be produced (1 mark) b. Explain how the data shown on the graph could be used to identify the limiting reagent in the reaction being studied. Answer: - When you graph the data, the amount of potassium iodide produced increases, and so does the mass of iron (ii) nitrate until no more lead iodide is produced, because all of the potassium iodide is consumed in the reaction. This would mean that all the potassium iodide has completely reacted and it would be the limiting reagent. Assignment Questions 1. 25.0 mL of 0.150-mol/L KBr(aq) is mixed with excess Pb(NO
3
)
2
(aq). (2 marks) a. Write the balanced chemical equation for this reaction. Answer: 2KBr(aq) + Pb(NO
3
)
2
(aq) -> 2KNO
3
(aq) + PbBr
2
(s) (2 marks) b. Calculate the number of moles of the limiting reagent. Answer: n(KBr) = 0.0250L × 0.150 mol/L = 0.00375mol (1 mark) c. Predict the number of moles of precipitate. Answer: N(PbBr
2
) = 0.00375/2 = 0.001875 mol (2 marks) d. Calculate the mass of precipitate. Answer: m(PbBr
2
)= (0.001875 mol)(367.01g/mol) = 0.690g 2. 3.00 L of methane, CH
4
(g), is combusted with 5.50 L of oxygen gas. Assume SATP conditions. (2 marks) a. Write the balanced chemical equation. Answer: CH
4
(g) + 2O
2
(g) -> CO
2
(g) + 2H
2
O(l) (2 marks) b. Determine the number of moles of each reactant. Answer: CH
4
(g) + 2O
2
(g) → CO
2
(g) + 2H
2
O(l) 3.00 L 5.50 L
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Related Questions
alibri (Body)
12
A A
Aa v
AaBbCcDc AaBbCcDc AaBbC AABBCCC AaB AABBCCD
IU abe x, x
A
ab
T Normal
T No Spac. Heading 1
Heading 2
Title
Subtitle
Font
Paragraph
Styles
3
6 IZICIt iniED 10 11 12
13 I 14 I-
15
16 .
Chemical Equation
Write a balanced equation that describes each of the following chemical reaction.
1. Acetylene gas, C2H2, burns in air forming gaseous carbon dioxide and, CO2, and water.
Answer: 2C2H2 + 502 → 4CO2 + 2H20 (double displacement/Combustion reaction)
2. MnO2 + KOH + O2 → H20 + K2MNO4
3. FeCl2 + Cl2 → FeCl3
English (United States)
Accessibility: Good to go
a
ENG
REDMI NOTE 10 PRO | JHANG
01/06/2022 15: 12
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Chemical Reaction Experiments: Coke and Mentos
1. The first bottle has 100 ml of coke and 1 piece of mentos.
2. The second bottle has 100 ml of coke and 3 pieces of mentos.
3. The third bottle has 100 ml of coke and 10 pieces of mentos.
Give your observations and why chemical reactions occurred.
arrow_forward
two partners were trying to solve the equation. Penny Said that the equation is balanced because there is only 1 Fe on both sides of the equation. But Alex disagrees. Who is correct and why? Write the CER to explain your answer. claim: Evidence: Reasoning
arrow_forward
2 Fe + Oz →2 FeO
1. The chemical in the pink box is a...
A. subscript
B. coefficient
C. reactant
D. product
2. The number in the green box is a...
A. subscript
B. coefficient
C. reactant
D. product
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Table 1. Heat of neutralization data
Sample 1
Sample 2
[1] Volume of HCl (mL)
50.1
50.2
[2] Temperature of HCl (°C)
24.3
25.0
[3] Volume of NaOH (mL)
49.9
50.1
[4] Temperature of mixture after reaction (°C)
31.0
Table 3. Heat of neutralization data and calculations
Sample 1
Sample 2
[1] Volume of HCl (mL)
50.1
50.2
[2] Temperature of HCl (mL)
24.3
25.0
[3] Volume of NaOH (mL)
49.9
50.1
[4] Temperature of mixture after reaction (°C)
31.0
31.7
Temperature difference (°C)
[5] Number of calories evolved (cal) enter a positive value
[6] Moles of H+ that were neutralized (mol)
[7] Calories evolved per mole of H+ (cal/mol)
arrow_forward
Which of the following is always correct in considering the percentage yield of a reaction?
There are cases that percentage yield is greater than 100%.
There are cases that percentage yield is greater than 100%.
Theoretical yield is always greater than actual yield.
Theoretical yield is always greater than actual yield.
There is no relationship between actual and percent yield.
There is no relationship between actual and percent yield.
Percent yield is derived from pre and post lab experiments.
Percent yield is derived from pre and post lab experiments.
Actual yield is always greater than theoretical yield.
Which of the following is always correct in considering the percentage yield of a reaction?
There are cases that percentage yield is greater than 100%.
There are cases that percentage yield is greater than 100%.
Theoretical yield is always greater than actual yield.
Theoretical yield is always greater than actual yield.
There…
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rmal text
BIUA
Arial
17.2
+
. 1. .
2. | 3 | 4
in blue ink using complete sentences.
1. How is a physical change different from a chemical change?
2. How do you know a chemical reaction has happened?
3. Give an example of a chemical change.
4. How do you know this chemical reaction has taken place?
5. Name three different properties you can test before and after a chemical reaction
to determine if a new substance was formed.
6. What does a catalyst do in a chemical reaction?
7. Are the number of atoms before and after a chemical reaction the same? Why?
8. What are two ways you can tell that the steel wool in the video underwent a
chemical reaction?
Support | Schoology Blog | PRIVACY POLI
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A. REACTIONS OF HYDROCARBONS
Three hydrocarbon samples were analyzed by various qualitative tests and the summary of their reactions is given in Table 1 below. Identify each unknown sample by matching the respective reaction profile with the given structures (A, B, or C).
Table 1. Summary of Reactions of Hydrocarbon Samples
Sample
Br2 in CCl4
KMnO4 in NaOH
AgNO3 in NH3
1
Fading of reddish-brown color
Brown precipitates
No reaction
2
Fading of reddish-brown color
Brown precipitates
Silver precipitates
3
Fading of reddish-brown color
No reaction
No reaction
Sample
Identity and Rationalization
1
2
3
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observation:
2
B. Balanced chemical equation:
C Calculation Do
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For numerical calculations, show all work with units in each step. Report final values to correct sig figs
with correct units.
1. Explain the difference between equivalence points and end point.
2. Write the chemical formula of acetic acid and then calculate its molar mass.
3. Write the balanced chemical equation between acetic acid and sodium hydroxide solution.
Include states for all reactants and products.
4. How many milliliters of 1.50 M NaOH are required to prepare 500.0 mL of 0.785 M NaOH
solution? State the dilution equation and show all related work.
5. Our primary standard is potassium hydrogen phthalate. This is abbreviated as KHP, which is
NOT its formula.
a.
Write the chemical formula of KHP and calculate its molar mass.
b. Calculate the molarity of sodium hydroxide solution if 31.45 mL are needed to titrate 0.6570
g…
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TYPES OF CHEMICAL REACTIONS DATA AND OBSERVATIONS
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Part C
Pbl
Express your answer as an ion.
Submit
ΑΣΦ
A chemical reaction does not occur for this question.
Part D
Request Answer
AIP
Express your answer as an ion.
?
ΑΣΦ
?
A chemical reaction does not occur for this question.
Submit Request Answer
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A. REACTIONS OF HYDROCARBONS
Three hydrocarbon samples were analyzed by various qualitative tests and the summary of their
reactions is given in Table 1 below. Identify each unknown sample by matching the respective reaction
profile with the given structures (A, B, or C).
Table 1. Summary of Reactions of Hydrocarbon Samples
Sample
Brz in CCI4
KMNO, in NaOH
AGNO3 in NH3
Fading of reddish-
brown color
Brown precipitates
1
No reaction
Fading of reddish-
brown color
Brown precipitates
Silver precipitates
3
Fading of reddish-
No reaction
No reaction
brown color
H3C
`CH3
H,C
CH3
А
Sample
Identity and Rationalization
1
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How many moles of W are needed to react with 1.0 mol of Ho in the hypothetic chemical reaction?
3W + 2Ho → 2W3Ho
a.
0
b.
1.5
c.
2
d.
3
e.
1
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Part B
BH?
Express your answer as a chemical formula.
Fo
ΑΣΦ
0
?
A chemical reaction does not occur for this question.
Submit
Request Answer
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In the PHET simulation, click on the Game icon at the bottom of the screen. Balance the given chemical equations by changing the coefficients placed before each compound and then clicking Check. When a reaction is balanced
correctly a yellow face will appear with a smile.
After practicing with the game, balance the given chemical equations without use of the simulation.
Drag the appropriate labels to their respective targets. Leave the target empty for a coefficient of 1.
> View Available Hint(s)
Reset
Help
3
H,C,0.
NaOH
Na,C,0,
H,0
5
Fe, 0,
Fe
CO
7
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MISSED THIS? Read Section 3.10 (Pages 118 - 123); Watch
IWE 3.18.
Calculate the empirical formula for each of the following
stimulants based on their elemental mass percent composition.
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just need the balanced equation and the two other blanks. this is a pre test that isn’t graded.
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What is the balanced net equation? It's unclear on my side. I only see 2 equations
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According to the following reaction, how many grams of water will be formed upon the complete reaction of 31.3 grams of oxygen
gas with excess hydrogen sulfide?
2H₂S(g) + 302(g) → 2H₂O(l) +2SO2(g)
9 water
Submit Answer
[Review Topics]
[References]
Use the References to access important values if needed for this question.
Mastered
Retry Entire Group 1 more group attempt remaining
Cengage Learning Cengage Technical Support
Previous
Next
Email Instructor Save and Exit
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Multiple Choice. Read and analyze each question. Write the letter that
corresponds to your answer on a separate sheet of paper.
1. Suppose your classmates will be visiting you. You decided to make burger for their
snack. You have 20 burger patties and 17 burger buns, how many burgers you can
make?
а. 20
b. 17
с. 3
d. 37
2. Based on problem 1, what is the limiting reactant?
a. burger buns
b. burger patties
c. your classmates
d. your budget
3. Based on problem 1, how many burger patties are extra after your preparation for
snack?
с. 17
d. 3
a. 0
b. 37
For numbers 4-10. If 68 g of Zn reacts with 27.5 g of HC1. Use the chemical equation
to answer the following questions below.
Zn + 2HC1
ZnCl2 + H2
4. What is the molar mass of Zn?
a. 65 g/mol
b. 30 g/mol
c. 27 g/ mol
d. 68 g/ mol
5. What is the molar mass of HC1?
a. 2 g/mol
b. 16 g/mol
6. What coefficient is indicated in HCl?
c. 36 g/mol
d. 68 g/mol
c. 4
d. 5
a. 2
b. 3
7. Which substance is limiting reactant?
a. ZnCl2
b. HCl
8. Which…
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18. Aniline to phenylisocyanide
19. Styrene to benzoic acid
20. Oxidation of acetone
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A. 26.0
B. 21.3
C. 22.5
D. 23.7
E. 24.8
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5 LAB QUESTIONS
5.1.1 Use the chemical equation below as a reference to answer part a and b of this question.
Cuo(s) + 2CH3COOH(aq)
Cu)+2CH3C00-
12+ + 2CH3COO¯ (aq) + H₂O (1)
a) This reaction took place in what step in of the experiment? What observation leads you to believe this?
This reaction took place when the penny was mixed with the acetic acid, this lead me to believe the structure of Cu^2+ which is aqueus
and CH300^- ions which is also aq.
b) Is copper being oxidized, reduced, or neither in this reaction? Explain.
Copper being that it is a solid goes to a ag ion state, which tells me the copper is being reduced during the reaction.
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In the PHET simulation, click on the Game icon at the bottom of the screen. Balance the given chemical equations by changing the coefficients placed before each compound and then clicking Check. When a reaction is balanced
correctly a yellow face will appear with a smile.
After practicing with the game, balance the given chemical equations without use of the simulation.
Drag the appropriate labels to their respective targets. Leave the target empty for a coefficient of 1.
• View Available Hint(s)
Reset
Help
3
NaOH
O Na,C,0,
4
H,C,0,
Fe, 0,
Fe
co2
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A. 15
B. 20
C. 18
D. 24
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moles. Enter all values with three digits (like shown) and include negative or positive signs for
the "Change" row.
A + 2B
ЗС + D
A
C
INITIAL
5.00
2.00
0.00
0.00
CHANGE
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Question 49
In 1-2 sentences, explain what the Arrhenius equation tells us. Use the diagram to help describe what you mean.
100 °C
-
room temperature
(300 °K)
k, = Ae¯FalRT
(373 °K)
4 kJ/mol
(1 kcal/mol)
40 kJ/mol
(10 kcal/mol)
80 kJ/mol
(19 kcal/mol)
→ energy (E)
Edit Format Table
12pt v Paragraph v BI Ų Av ev T? v * s
fraction of molecules
having energy E
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chemistry reaction questions
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2 KClO3 → 2 KCl + 3 O2How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely? *
1.0 mol
4.5 mol
6.7 mol
10.1 mol
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Now let's use these total masses to figure out how much CO2 was generated by the experiment.
Remember, the amount of CO2 generated is the mass lost after the reaction, all of the other products
are still in the cups. Calculate both the grams and moles of CO2.
Sample Data for Vinegar Lab
Total Mass of
Total Mass of
Baking Soda & Baking Soda &
g CO2 Produced by moles CO2 Produced by
Vinegar Cups Vinegar Cups (g,
post)
Reaction
Reaction
(g, pre)
-2 g
56.94
44.26
NaHCO3
-4 g
59.59
57.55
NaHCO3
-6 g
63.37
61.07
NaHCO3
-8 g
66.68
64.58
NaHCOз
-10 g
69.81
67.66
NaHCO3
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Law of conservation of mass within a chemical Equation
Please write an balanced equation
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HSC 258
Major Projec X
Mind Tap - Cengage Lea X
d%3D55750828934189288909969212&elSBN=9781305657571&snapshotld%3D219989
The illustration to the left represents a mixture of
iodine ( purple ) and fluorine ( green )
molecules.
If the molecules in the above illustration react to form IF3 according to the equation
I +3 F2 2 IF3 ,
the limiting reagent is
the number of IF, molecules formed is
and
the number of
atoms/molecules in excess is
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