Lab 6 Alka Seltzer Strength_Spring2024
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Spring 2024
Lab 6 Assignment: Alka Seltzer Strength
Be sure to report all data and calculated results with the correct number of significant figures. Record all digits when making measurements. Follow the rules for significant figures
, and remember that the rules for addition and subtraction differ from the rules from multiplication and division.
Part 1: Determining the Nature of the Reaction
1. Based on the Background information, what product of the reaction causes the bubbling to occur when Alka-Seltzer is added to the vinegar?
The product of the reaction causing the bubbles is the carbon dioxide gas or CO2.
2. Based on the Background information, what component of Alka-Seltzer reacts with the acid in the vinegar? Write its name and chemical formula.
Sodium Bicarbonate – NaHCO3
3. Use the Background information and Chapter 4 in your textbook as a reference to write a balanced equation (including physical states) for the reaction you observed when you added sodium bicarbonate to the acid in vinegar, acetic acid, HC
2
H
3
O
2
(
aq
). NaHCO3(s)+HC2H3O2(aq)→H2O(l)+CO2(g)+NaC2H3O2(aq)
4. Explain why the other components of Alka-Seltzer (described in the Background) should not react with acetic acid in vinegar to product a gas.
The other components of Alka-Seltzer don’t have the necessary components to participate in the acid-
base neutralization reaction therefor they don’t react with anything in the reaction.
Page 1
of 7
Name: Cody Kaiser
Date: 4/18/24
5. Fill in the table below with your recorded data and calculated results for Part 1.
BEAKER Column (1)
Initial Mass
(g)
Column (2)
Final Mass
(g)
Column (3)
Mass CO
2
evolved (g)
Column (4)
Moles
CO
2
evolved
(mols)
#
Mass of beaker & solution (g)
Mass of Alka-
Seltzer (g)
1
67.089g
2.000g
69.089g
68.500g
.589g
.0134 moles
Column 1: This initial mass
(before reaction) is the measured mass of the beaker containing the vinegar solution PLUS the mass of the Alka-Seltzer tablet (2.000 g). Column 2: This final mass
is the measured mass of the beaker with its solution after the reaction between the Alka-Seltzer with the vinegar. Column 3: Calculate the mass of CO
2
evolved in each beaker by subtracting the final mass from the initial mass.
Show calculation for Beaker #1 here.
69.089g-68.500g = .589g
Column 4: Convert the mass of CO
2
evolved (column 3) to moles of CO
2
evolved. When determining molar mass of CO
2
, be sure to use at least four significant figures in your molar mass values obtained from the periodic table. For Beaker #1, write the value for mass of CO
2
evolved and show your calculation here.
.589g / (44g/mol) = .0134 mols
6. Which of the following statements is true? Circle or highlight your choice.
A.
The moles of the CO
2
gas evolved should be equal to the moles of the NaHCO
3
(in the Alka-
Seltzer tablet) that reacted.
B.
The mass of the CO
2
gas evolved should be equal to the mass of the Alka-Seltzer tablet.
C.
The moles of the CO
2
gas evolved should be less than the moles of the NaHCO
3
(in the Alka-
Seltzer tablet) that reacted.
D.
The mass of the CO
2
gas evolved should be equal to the mass of the NaHCO
3
in the Alka-Seltzer tablet.
Page 2
of 7
Part 2: Determining the Percent-By-Mass NaHCO3 in Alka-Seltzer
Be sure to report all data and calculated results with the correct number of significant figures. Record all digits when making measurements. Follow the rules for significant figures
, and remember that the rules for addition and subtraction differ from the rules from multiplication and division.
7. Fill in the table below with your recorded data and calculated results. More descriptive instructions for each column are below the chart. For some of the columns you’ll need to show a sample calculation.
BEAKER
#
Column (1)
Initial Mass
(g)
Column (2)
Final Mass
(g)
Column (3)
mass CO
2
evolved (g)
Column (4)
moles CO
2
evolved (mols)
Column (5)
moles of
NaHCO
3
reacted (mols)
Column (6)
mass of
NaHCO
3
reacted (g)
1
65g
64.239g
.761g
.0173 mols
.0173 mols
1.453g
2
65.005g
64.171g
.834g
.0190 mols
.0190 mols
1.596g
3
65.010g
64.127g
.883g
.0200 mols
.0200 mols
1.681g
4
65.015g
64.132g
.883g
.0200 mols
.0200 mols
1.681g
5
65.020g
64.137g
.883g
.0200 mols
.0200 mols
1.681g
6
65.026g
64.172g
.854g
.0194 mols
.0194 mols
1.630g
Column 1: This initial mass
(before reaction) is the measured mass of the beaker containing the water and vinegar PLUS the mass of the Alka-Seltzer tablet (3.000 g). Column 2: This final mass
is the measured mass of each beaker with its solution after the reaction
between the Alka-Seltzer with the vinegar and water. Column 3: Calculate the mass of CO
2
evolved in each beaker by subtracting the final mass from the initial mass.
Show calculation for Beaker #6 here.
65.026g – 64.172g = .854g
Column 4: Calculate the number of moles of CO
2
evolved in each beaker. (Remember to use molar mass
with at least four significant figures in your calculation.) Write the value and show calculation for Beaker #6 here.
Page 3
of 7
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Related Questions
Name
Lab Partner
Section #
Date
Pre-Lab Assignment: Stoichiometry Lab
1.
In a lab experiment similar to the one you are going to do, a student slowly added hy-
drochloric acid (HCI) to an evaporating dish containing magnesium carbonate MgCO3.
a. Complete and balance the following equation for the reaction between magnesium
carbonate and hydrochloric acid.
MgCO3 (s) + HCl (aq) →
(aq) + H₂CO3(aq)
(When writing the formula for the missing product did you consider the charges
of the ions?)
b. When carbonic acid is formed in a chemical reaction, it is unstable and immedi-
ately decomposes into carbon dioxide and water. Rewrite the equation above to
show the final products using this information.
arrow_forward
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
arrow_forward
If this item does not open automatically you can open Data Sheet here
=
106106334
Part I. Reaction of Fe³+ and SCN™
Test tube
A
B
C
5
Adding NH3 (aq)
1/1
Action performed
Experiment 15
Chemical Equilibrium and Le Châtelier's Principle
Adding Fe(NO3)3 (aq)
Adding NaSCN (aq)
Adding NaNO3(aq)
Part II. Reaction of Cu²+ and aqueous NH3
Action performed
Mixing CuSO4 and NH3 (aq).
Oll
y
31
88% +
Data Sheet
Observations
Observations.
DELL
العال[
O
:
*
8
CH127 Introductory General Chemistry Laboratory
Conclusion
Conclusion
O
Dec 18
8:09 2
3
Р
arrow_forward
Post- Lab
Write the correct formula of the products and balance each equation.
A. Instructor Demonstration- Combination reaction
Reactants
Products
Mg (s) + O, (g) Magnesium oxide (s)
Balanced equation:
arrow_forward
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
arrow_forward
19. The chemical equation for photosynthesis is
_CO2 (g) + _H₂O (1)→ __C6H1206 (s) +
(C6H12O6 is glucose, the simplest sugar)
a. Balance the chemical equation above by filling in the blanks.
b. According to onetreeplanted.org, the average tree (across all climates and sizes) removes 10 kg of
carbon dioxide from the atmosphere every year. Based on this, what mass of glucose is produced
annually by the average tree?
O2 (g)
c. Teak is a common species of tropical tree. The graph below shows the amount of CO₂ absorbed by teak
forests in tons of CO₂ per hectare of forest per year, according to the climate region where the forests
are found (dry = low rainfall, humid=high rainfall). Looking at your photosynthesis equation again, what
does this data suggest about which reactant is the limiting reactant for teak trees? Explain.
C Teak
Carbon sequestration rate (tons CO₂ ha -1yr -1)
10
10
20
Tropical
humid
Tropical
dry
Aboveground biomass,
0-20 years
Belowground biomass,
0 -20 years
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maining Time: 1 hour, 01 minute, 27 seconds.
uestion Completion Status:
A Moving to another question will save this response.
estion 33
For Questions 30-35:
Nitric acid is prepared from the reaction of 69.0 grams of nitrogen dioxide with 36 grams of water.
unbalanced chemical equation:
NO2 + H₂O → HNO3 + NO
How many grams of NO are produced?
60 g
45 g
30 g
15 g
Moving to another question will save this response.
4
144
arrow_forward
12. Name each chemical and complete the reaction
↑ Add file
+
H₂O
arrow_forward
CHEMISTRY 1110L
LAB REPORT: REACTIONS OF COPPER (Part B)
1. Reaction 4:
a. Color of copper(II) sulfate
b. Water solubility of copper(II) sulfate
2. Reaction 5:
CuO + H₂SO4 →
CuSO4 +
Zn →>>
-
5. Percent recovery
(calculations)
3. Mass of copper metal recovered
4. Initial mass of copper (from Part A)
CuSO4 +
Cu +
ZnSO4 +
Zn + H₂SO4
a. Color of zinc metal (before reaction)
b. Color/appearance of copper metal (after reaction)
c. Color of solution before reaction
d. Color of solution after reaction
e. Color of hydrogen gas
ZnSO4
H₂O
blue Solid
Water
6. Initials of instructor or teaching assistant (TA) own
H₂
Name
• Loona Alg busi
Partner
Desk #
AR
Solid metal-normal color
20
arrow_forward
Mg + 2HCl → MgCl2 + H2
This experiment was performed two times.
All values are valid to one decimal place. If the decimal place is not shown, add a ".0"
Experiment Mass of Mg (mg) Starting Temperature (°C) Final Temperature (°C)
1
2
19.6
20.7
19.5
20.7
33
33.5
The previous page contained data from two experimental runs for the reaction between magnesium and
hydrochloric acid.
Mg+ 2HC! MgCl2 + H2
First, how many moles (n) of Mg reacted with the HCI? Use the average value of the two masses from
your provided data set.
Answer: 0.001658
I
Mg + 2HCI MgCl2 + H2
Next, what is the amount of heat absorbed by the water (qsurr) in the experiment? Use the average AT
from your data to calculate a single value for q. Report your answer in J.
Remember to consult the lab manual and/or the video for any values you might need.
Answer:
Mg + 2HC! MgCl2 + H2
Finally, calculate A,H for this reaction and report your answer in kJ/mol.
Answer:
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Balance the following chemical equation by placing a coefficient (including 1) in each answer box that is in front of each reactant and each product.
While coefficients that are equal to 1 are not placed in front of either a reactant or product, you MUST include any coefficient that is equal to 1 in this
problem.
type your answer...
C₂H12 +
type your answer...
2
type your answer...
CO₂ +
type your answer...
H₂O
arrow_forward
IDENTIFYING SYNTHESIS REACTIONS
GAOW
Tên equations are listed below. Some are synthesis reactions, Some are not. Make a check (/) in
the correct box next to each equation.
Not a
Equation
Synthesis
Reaction
Synthesis
Reaction
1.
2K + Br, – 2KB1
2.
2H,0
2H, + O,
-
3.
Nacl
Na + Cl
4.
4Au + 30,
2Au,0,
5.
2Na + 2HCI
→ 2NACI + H,
Cu + Br,
CuBr,
>
7.
Zn + S ZnS
8.
2NA + Br,
→ 2NAB.
9.
2H8O
2Hg + O,
>
10.
2Na + 1,
2Nal
6.
arrow_forward
Given the combustion reaction below, how many moles of CO2 are formed given that you start with 1.50 x 10^-2 mol of C3H8O. (Assume O2 is in excess).
2 C3H8O + 9O2 ---> 6 CO2 + 8 H2O
A. 3.00 x 10^-2 mol
B. 4.50 x 10^-2 mol
C. 5.00 x 10^-3 mol
D. 7.50 x 10^-3 mol
E. none of the above
arrow_forward
Chemical Reactions and Equations
3. Observation of burning match or splint.
What caused the change in the burning match or splint?
4.
Na,CO3(s)+
HCl(aq)
» CO, (g)+
H2O(1)+ NaCl(aq)
5. Type of reaction:
F. Hydrogen Peroxide
Reactants
1. Appearance of
Reactants
2. Evidence of a Chemical
Reaction
H,O2(aq)
3.
H2O¿(aq) – KI
H2O(1) +.
O2(g)
4. Type of chemical reaction:
Questions and Problems
Q1 What evidence of a chemical reaction might you see in the following cases? Refer
to Table 1.
a. dropping an Alka-Seltzer tablet into a glass of water
b. bleaching a stain
c. burning a match
d. rusting of an iron nail
Q2 Balance the following equations:
a. Mg(s) + HCl(aq)
H2(g)+.
MgCl2 (aq)
b.
Al(s) +
02(g)
Al,O;(s)
89
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a.The stoichiometric coefficient of a compound is the number in front of the compound in the reaction formula. The coefficient is negative for a reactant and positive for a product.b.Reaction heat is the heat development that occurs during a chemical reaction.c.When a gas is heated, the enthalpy content decreases.d.Entalpine changes during phase transformation (for example when iron melts or water evaporates).e.In an endothermic reaction, heat develops.
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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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O Launch Meeting - Zoom
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A honeycomb-shape casing of the metals platinum (Pt), rhodium (Rh), and palladium
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They cause the reactions without being affected.
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Complete the ICF (BCA) table below for the hypothetical chemical reaction. All values are in moles. Enter all values with three digits (like shown) and include negative or positive signs for the "Change" row.
A + 2B
3C + D.
INITIAL
CHANGE
FINAL
A
5.00
4.00
B
2.00
0.00
C
0.00
D
0.00
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Then use the controls below to enter your equation and check your answer.
Reactants
Add Reactant
Products
Add Product
Preview:
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Balance the reaction shown below:
H2CO3+NaOH→Na2CO3+H2OH2CO3+NaOH→Na2CO3+H2O
Once balanced, given 0.367 moles H2CO3H2CO3, calculate the grams of H2OH2O produced.
A. 1.65
B. 38.3
C. 13.2
D. 61.8
E. 16.9
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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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Based on the process below, how many
moles of electrons are transferred during
the reaction?
3Pb(s) + 2Cr3+ (aq) = 3Pb²+ (aq) + 2Cr(s)
n = [?] moles of e-
moles of electrons
Enter
Copyright © 2003-2022 International Academy of Science. All Rights Reserved.
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Predict he products and balance the chemical equation involving decomposition reaction. Have photo of your answers and attach it at the
box below. Accepts pdf and jpg only. Use a darker pen.
Decomposition Reaction
1. Fe,0,
2. Sodium chlorate
3. Magnesium carbonate
4. MgSO4, 7 H,0
5. NaHCO,
Single Displacement Reaction
1. Na + Cas
2. Li + Bao|
heat
3. Ва + H,0
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A LEAP 2025 Prep in 8th Grade Sci x
s.com/r/s/0/doc/607216/sp/179325173/mi/571531285?cfi=%2F4%2F4
Chapter 7 Key Terms Activity
Word Bank
covalent
ionic
atoms
ions
reactants
molecules
bonding
gains
products
share
cation
equation
reaction
anion
form 2.
or compounds through 3.
during a chemical 4.
The best way to express this reaction is with a chemical
5.
In this expression, you can show how 6.
result into
7.
Some of the reactions involve 8,
in which a(n)
and a(n) 10.
form a neutral product. The atoms form
9.
bonds in which one atom 12.
an electron and another
11
atom 13
an electron, 14
bonding occurs when atoms
15.
electrons.
Key terms are defined in the book's glossary. Answers to Key Term Activities and chapter
reviews are found in the Teacher's Cuide
Teachers, remember there is a review test for your use in the Teacher's Guide
hp
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What is the missing particle in the reaction below? 27/13 Al +1/1 H → 27/14 Si + ?
A.
e
B.
n
C.
He
D.
H
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emaining Time: 1 hour, 05 minutes, 35 sečonds.
Question Completion Status:
A Moving to the next question prevents changes to this answer.
Question 2
How many moles of Fe203 will be produced from the complete reaction of 1.57 moles of O2 as described in the following equation:
4Fe + 30, → 2Fe203
A Moving to the next question prevents changes to this answer.
a
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enter
V || B N
pause
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立
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Please help me how to solve this equation. Thank you very much.
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In part 1 of this lab, you will be calculating A₁H by conducting constant-pressure calorimetry
measurements.
One of the final steps in this calculation is obtaining ArH by taking the q value (with respect to the
system) and dividing by n.
What number of moles (n) will you be using in the above formula?
Select one:
Number of moles of magnesium, since Mg is in the balanced chemical equation and is a part of the
system
Number of moles of water
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CABOR
Page
12
> ar65
ZOOM
Learning Check
Balance each equation.
А.
Mg(s)
+__N2(g)
→_M93N2(s)
В.
Al(s)
+_Cl,(g) →_AICI3(s)
BF3(g)
+_H20(1) →_B203(aq) +_HF(aq)
D.
Fe203(s) +__C(s)
_Fe(s)
+__CO2(g)
E. Al(s)
+
Fe0(s)
_Fe(s)
+_Al,03(s)
184
RO
DE
G
B.
LL
C.
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Using your reaction page, predicte the products and balance the reation. What type of reaction would the following be ID as?
KCI(aq) + NaNO3(ag) →?
Comb. #1
no reaction
Comb. #4
Comb. #2
Double Replacement
Decomp. #5
Single Replacement #1
Decomp. #2
Decomp. # 1
Single Replacement # 2
Total Combustion of a Hydrocarbon
Comb. #3
Decomp. #4
Decomp. #3
hp
C
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%
&
3.
4
8
9.
AU
S
d.
m
OO00 O O O O
O O O O
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Predict the products of the reaction below. That is, complete the right-hand side of the chemical equation. Be sure your equation is balanced.
HI + NaOH →
I Don't Know
1841
Submit
3
E
5
T
6
G
0-0
X
S
stv♫
5
© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Cer
A
all
9
zoom
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What is the molar mass of each of the following compounds? Show all work.a. Ru(NH3)6Cl3b. WO2c. PbI2
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2 Fe + Oz→2 FeO
The chemical in the pink box is a...
A. subscript
B. coefficient
C. reactant
D. product
The number in the green box is a...
A. subscript
В. соefficient
C. reactant
D. product
The numbers in red boxes are...
A. subscripts
В. соeficients
C. reactants
D. products
The chemicals in the purple box are...
A. subscripts
В. соefficients
C. reactants
D. products
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Plz do the 4 and 5 of level 2... for each one write the chemical reaction in symbols... highlight the coefficients...
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- Name Lab Partner Section # Date Pre-Lab Assignment: Stoichiometry Lab 1. In a lab experiment similar to the one you are going to do, a student slowly added hy- drochloric acid (HCI) to an evaporating dish containing magnesium carbonate MgCO3. a. Complete and balance the following equation for the reaction between magnesium carbonate and hydrochloric acid. MgCO3 (s) + HCl (aq) → (aq) + H₂CO3(aq) (When writing the formula for the missing product did you consider the charges of the ions?) b. When carbonic acid is formed in a chemical reaction, it is unstable and immedi- ately decomposes into carbon dioxide and water. Rewrite the equation above to show the final products using this information.arrow_forwardA. 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 1arrow_forwardIf this item does not open automatically you can open Data Sheet here = 106106334 Part I. Reaction of Fe³+ and SCN™ Test tube A B C 5 Adding NH3 (aq) 1/1 Action performed Experiment 15 Chemical Equilibrium and Le Châtelier's Principle Adding Fe(NO3)3 (aq) Adding NaSCN (aq) Adding NaNO3(aq) Part II. Reaction of Cu²+ and aqueous NH3 Action performed Mixing CuSO4 and NH3 (aq). Oll y 31 88% + Data Sheet Observations Observations. DELL العال[ O : * 8 CH127 Introductory General Chemistry Laboratory Conclusion Conclusion O Dec 18 8:09 2 3 Рarrow_forward
- Post- Lab Write the correct formula of the products and balance each equation. A. Instructor Demonstration- Combination reaction Reactants Products Mg (s) + O, (g) Magnesium oxide (s) Balanced equation:arrow_forwardA. 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 3arrow_forward19. The chemical equation for photosynthesis is _CO2 (g) + _H₂O (1)→ __C6H1206 (s) + (C6H12O6 is glucose, the simplest sugar) a. Balance the chemical equation above by filling in the blanks. b. According to onetreeplanted.org, the average tree (across all climates and sizes) removes 10 kg of carbon dioxide from the atmosphere every year. Based on this, what mass of glucose is produced annually by the average tree? O2 (g) c. Teak is a common species of tropical tree. The graph below shows the amount of CO₂ absorbed by teak forests in tons of CO₂ per hectare of forest per year, according to the climate region where the forests are found (dry = low rainfall, humid=high rainfall). Looking at your photosynthesis equation again, what does this data suggest about which reactant is the limiting reactant for teak trees? Explain. C Teak Carbon sequestration rate (tons CO₂ ha -1yr -1) 10 10 20 Tropical humid Tropical dry Aboveground biomass, 0-20 years Belowground biomass, 0 -20 yearsarrow_forward
- maining Time: 1 hour, 01 minute, 27 seconds. uestion Completion Status: A Moving to another question will save this response. estion 33 For Questions 30-35: Nitric acid is prepared from the reaction of 69.0 grams of nitrogen dioxide with 36 grams of water. unbalanced chemical equation: NO2 + H₂O → HNO3 + NO How many grams of NO are produced? 60 g 45 g 30 g 15 g Moving to another question will save this response. 4 144arrow_forward12. Name each chemical and complete the reaction ↑ Add file + H₂Oarrow_forwardCHEMISTRY 1110L LAB REPORT: REACTIONS OF COPPER (Part B) 1. Reaction 4: a. Color of copper(II) sulfate b. Water solubility of copper(II) sulfate 2. Reaction 5: CuO + H₂SO4 → CuSO4 + Zn →>> - 5. Percent recovery (calculations) 3. Mass of copper metal recovered 4. Initial mass of copper (from Part A) CuSO4 + Cu + ZnSO4 + Zn + H₂SO4 a. Color of zinc metal (before reaction) b. Color/appearance of copper metal (after reaction) c. Color of solution before reaction d. Color of solution after reaction e. Color of hydrogen gas ZnSO4 H₂O blue Solid Water 6. Initials of instructor or teaching assistant (TA) own H₂ Name • Loona Alg busi Partner Desk # AR Solid metal-normal color 20arrow_forward
- Mg + 2HCl → MgCl2 + H2 This experiment was performed two times. All values are valid to one decimal place. If the decimal place is not shown, add a ".0" Experiment Mass of Mg (mg) Starting Temperature (°C) Final Temperature (°C) 1 2 19.6 20.7 19.5 20.7 33 33.5 The previous page contained data from two experimental runs for the reaction between magnesium and hydrochloric acid. Mg+ 2HC! MgCl2 + H2 First, how many moles (n) of Mg reacted with the HCI? Use the average value of the two masses from your provided data set. Answer: 0.001658 I Mg + 2HCI MgCl2 + H2 Next, what is the amount of heat absorbed by the water (qsurr) in the experiment? Use the average AT from your data to calculate a single value for q. Report your answer in J. Remember to consult the lab manual and/or the video for any values you might need. Answer: Mg + 2HC! MgCl2 + H2 Finally, calculate A,H for this reaction and report your answer in kJ/mol. Answer:arrow_forwardBalance the following chemical equation by placing a coefficient (including 1) in each answer box that is in front of each reactant and each product. While coefficients that are equal to 1 are not placed in front of either a reactant or product, you MUST include any coefficient that is equal to 1 in this problem. type your answer... C₂H12 + type your answer... 2 type your answer... CO₂ + type your answer... H₂Oarrow_forwardIDENTIFYING SYNTHESIS REACTIONS GAOW Tên equations are listed below. Some are synthesis reactions, Some are not. Make a check (/) in the correct box next to each equation. Not a Equation Synthesis Reaction Synthesis Reaction 1. 2K + Br, – 2KB1 2. 2H,0 2H, + O, - 3. Nacl Na + Cl 4. 4Au + 30, 2Au,0, 5. 2Na + 2HCI → 2NACI + H, Cu + Br, CuBr, > 7. Zn + S ZnS 8. 2NA + Br, → 2NAB. 9. 2H8O 2Hg + O, > 10. 2Na + 1, 2Nal 6.arrow_forward
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