6-1 Ideal Gas Law Constant Lab Kristen Brown
docx
keyboard_arrow_up
School
Southern New Hampshire University *
*We aren’t endorsed by this school
Course
101L
Subject
Chemistry
Date
Jan 9, 2024
Type
docx
Pages
4
Uploaded by kb4410
Determination of Ideal Gas Law Constant
S
tudent: Kristen Brown
Date: 11/30/23
Activity 1
If your concentration, moles, or R calculations are incorrect or your calculation work does not actually result in
the desired final units, or units are missing/incomplete, or cancelled incorrectly, you will lose points. Be sure
that every number you include has its associated unit.
Email me if you are unsure or need assistance.
Data Table 1
Trial 1
(1 mL
H
2
O
2
)
Trial 2
(1 mL
H
2
O
2
)
Trial 3
(2 mL
H
2
O
2
)
Trial 4
(2 mL
H
2
O
2
)
Trial 5
(3 mL
H
2
O
2
)
Trial 6
(3 mL
H
2
O
2
)
Trial 7
(4 mL
H
2
O
2
)
Trial 8
(4 mL
H
2
O
2
)
Air temperature
(°C)
25°C
25°C
25°C
25°C
25°C
25°C
25°C
25°C
Volume H
2
O
2
liquid (mL)
1.0mL
1.0mL
2.0mL
2.0mL
3.0mL
3.0mL
4.0mL
4.0mL
Initial Volume
Gas (mL)
0.0mL
0.2mL
0.0mL
0.3mL
0.0mL
1.0mL
0.0mL
1.2mL
Final Volume
Gas (mL)
9.2mL
11.3mL
18.5mL
19.4mL
32.5mL
34.8mL
40.0mL
41.9mL
ΔV (mL)
9.2mL-
0.0mL =
9.2mL
11.3mL-
0.2mL =
11.1mL
18.5mL
-
0.0mL =
18.5mL
19.4mL
-
0.0mL =
19.1mL
32.5mL
-
0.0mL =
32.5mL
34.8mL
-
1.0mL =
33.8mL
40.0mL
-
0.0mL =
40.0mL
41.9mL
-
1.2mL =
40.7mL
©2016 2 Carolina Biological Supply Company
2021
Activity 2
Data Table 2
Show work for determining Concentration of H
2
O
2
in the box below. Concentration should be mol/L.
You
need to begin your calculation using the provided 3%m/v H
2
O
2
concentration
.
Concentration
H
2
O
2
(mol/L)
30.0g H
2
O
2
/ 1000mL
30.0g H
2
O
2
x 1.0mol H
2
O
2
/ 34.01g H
2
O
2
= 0.88mols H
2
O
2
/ L
Trial 1
1 mL H
2
O
2
Trial 2
1 mL H
2
O
2
Trial 3
2 mL H
2
O
2
Trial 4
2 mL H
2
O
2
Trial 5
3 mL H
2
O
2
Trial 6
3 mL H
2
O
2
Trial 7
4 mL H
2
O
2
Trial 8
4 mL H
2
O
2
Mole
s
H
2
O
2
0.0009mol
H
2
O
2
0.0009mol
H
2
O
2
0.0018mol
H
2
O
2
0.0018mol
H
2
O
2
0.0026mo
l
H
2
O
2
0.0026mo
l
H
2
O
2
0.0035mol
H
2
O
2
0.0035mol
H
2
O
2
Mole
s O
2
*
0.00045mo
l
O
2
0.00045mol
O
2
0.0009mol
O
2
0.0009mol
O
2
0.0013mo
l
O
2
0.0013mo
l
O
2
0.00175mo
l
O
2
0.00175mo
l
O
2
ΔV
(L)
1L =
1000mL
9.2mL
/1000 =
0.0092L
1L =
1000mL
11.1mL
/1000 =
0.0111L
1L =
1000mL
18.5mL
/1000 =
0.0185L
1L =
1000mL
19.1mL
/1000 =
0.0191L
1L =
1000mL
32.5mL
/1000 =
0.0325L
1L =
1000mL
33.8mL
/1000 =
0.0338L
1L =
1000mL
40.0mL
/1000 =
0.04L
1L =
1000mL
40.7mL
/1000 =
0.0407L
*Hint: Use reaction stoichiometry/molar ratio to solve for moles of O
2
.
Show work for determining moles of H
2
O
2
for Trial 1
here:
1.0mL H
2
O
2
x 1L/1000mL x 0.88mols H
2
O
2
/1L = 0.00088mols H
2
O
2
Show work for determining moles of O
2
for Trial 1
here:
0.0009mols H
2
O
2
x 1.0mol O
2
/2.0mols H
2
O
2
= 0.00045mols O
2
Show work for determining moles of H
2
O
2
for Trial 3
here:
2.0mL H
2
O
2
x 1L/1000mL x 0.88mols H
2
O
2
/1L = 0.00176mols H
2
O
2
Show work for determining moles of O
2
for Trial 3
here:
0.0018mols H
2
O
2
x 1.0mols O
2
/2.0mol H
2
O
2
= 0.0009mols O
2
Show work for determining moles of H
2
O
2
for Trial 5
here:
3.0mL H
2
O
2
x 1L/1000mL x 0.88mols H
2
O
2
/1L = 0.00264mols H
2
O
2
Show work for determining moles of O
2
for Trial 5
here:
0.0026mols H
2
O
2
x 1.0mol O
2
/2.0mols H
2
O
2
= 0.0013mols O
2
© 2016 Carolina Biological Supply Company
2021
Show work for determining moles of H
2
O
2
for Trial 7
here:
4.0mL H
2
O
2
x 1L/1000mL x 0.88mols H
2
O
2
/1L = 0.00352mols H
2
O
2
Show work for determining moles of O
2
for Trial 7
here:
0.0035mols H
2
O
2
x 1.0mol O2/2.0mols H
2
O
2
= 0.00175mols O
2
Insert a copy of your graph. Your graph must include the
equation of the line displayed, your name and date
in
the title.
You cannot complete the rest of this lab without this graph and the equation of the line. See the Week 6
Announcement for an example. Don’t forget to set the y-intercept to 0.
Graph:
0
0
0
0
0
0
0
0
0
0
0
0.01
0.01
0.02
0.02
0.03
0.03
0.04
0.04
0.05
f(x) = 23.45 x
Volume of O2 vs Moles O2
Kristen Brown 12/2/2023
Moles O2
Vol. O2 (L)
Show work,
including all units
, for the calculations/conversions for Air Temperature, Gas Constant R, and
Percent Error in the boxes below. Calculations must include complete units to be correct. This includes the
correct units for the slope.
Air Temperature (K)
Show work in the space
provided.
25°C + 273.15 = 298.15K
Air Pressure (atm)
Show work in the space
provided.
1 atm
Equation of the Line
Y = 23.451x
© 2016 Carolina Biological Supply Company
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
2021
Gas Constant R
Show work in the space
provided.
23.451 * l/mols * (1 atm)
/298.15 k
=
0.0787 L(atm)/mols(K)
Percent Error
Show work in the space
provided.
Use 0.0821 L*atm/mol*K in
your calculation
(|0.0821 L
∗
atm/mol
∗
K−0.0787 L
∗
atm/mols
∗
K|
/0.0821 L
∗
atm/mol
∗
K)
* 100
=
4.14% error
Question 1:
Would the volume of oxygen that is generated be affected if a smaller mass of yeast were used?
Why or why not?
Yes, if less yeast is used, there would be a smaller amount of catalase present to perform as the catalyst to the
decomposition of H
2
O
2
. This would directly result in a smaller amount of O
2
being produced.
Question 2:
Identify at least two potential sources of error in the experiment. Are any assumptions made that
would add to the experimental error?
Some potential sources of error would be the scale having trouble reading such low numbers. Another would be
how much gas is lost between the time of adding H
2
O
2
and putting the cap back on the bottle. Lastly, another
potential error could be if any residual liquid is still in the container from the previous trials.
© 2016 Carolina Biological Supply Company
Related Documents
Related Questions
Hi! I am unsure of how to solve this problem. Thank you!
arrow_forward
need help with qurstion
arrow_forward
2.) It’s a bad day in the lab! Two students are doing experiments. Each is 20 feet away from the professor. At the same time, each of them lets the same amount of a smelly gas into the room. One of them releases ammonia, NH3, and the other releases SO2. NH3 has a pungent odor, and SO2 smells like rotten eggs. The professor has no idea that this has happened, until she smell the first gas. Which chemical will the professor smell first? (NH3 or SO2) . If the professor starts to smell the first gas 42. seconds after the gas is released, how long will it take her to smell the second gas? sec.
* Note: It is unsafe practice to work with these chemicals in an open lab.
arrow_forward
AP Classroom Learning Checkp x
CD
PLSD Student
S
+
arrow_forward
Solve like the example.
arrow_forward
Help with these questions
arrow_forward
Only typed solution.
arrow_forward
Consider the general chemical equation: 2A+2B-->4C+D.
Part A. How many moles of C are produced from 2 mol of A?
Express your answer as an integer and include appropriate units.
Part B.
How many porters of gas B must react to give 1L of gas D at the same temperature and pressure?
express your answer as integer and include appropriate units.
arrow_forward
earson.com/?courseld=1
←
2
S
MISSED THIS? Read Section 4.2 (Page); Watch
KCV 4.2, IWE 4.2.
W
Write a balanced chemical equation for each
reaction.
म
X
→
#3
E
D
C
C
$
4
R
F
V
%
5
T
G
B
^
▾
6
Part A
G Search or type URL
Y
Aqueous hydrogen chloride reacts with oxygen gas to form chlorine gas and liquid water.
Express your answer as a chemical equation. Identify all of the phases in your answer.
² ΑΣΦ
H
Submit
Part B
A chemical reaction does not occur for this question.
Part C
Request Answer
Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water.
Express your answer as a chemical equation. Identify all of the phases in your answer.
Submit Request Answer
MacBook Pro
ΑΣΦ 4
A chemical reaction does not occur for this question.
&
7
N
Nitrogen monoxide gas reacts with hydrogen gas to form ammonia gas and water vapor.
Express your answer as a chemical equation. Identify all of the phases in your answer.
U
J
☆
* 00
B
8
M
C w ?
I
?
K
(
9.
<
O
)
- O
L
P
A
I'
Review I…
arrow_forward
hydroch
2. Unlike oxygen gas, nitrogen gas (the other major component of air) is generally unreactive. Magnesium is one metal
that can react with nitrogen directly. What volume of nitrogen gas, measured at a pressure of 1.00 atm and a
temperature of 27°C, will react with 5.0 g of magnesium?
Mg(s) + N2(g) → Mg3N2(s).
[unbalanced equation]
cas and hyd
what mass of ammon
mitroge
must decompose to
arrow_forward
江苏高考分数线
A
Acellus
Applications of the Ideal Gas Law
0.0453 moles of hydrogen gas were
produced by the reaction. Calculate the
volume of the gas at standard
temperature and pressure.
Mg + 2HCI → MgCl2 + H₂
Volume H₂ = [?]L
C
Liters of H₂
Enter
28
2
Resources
Help
arrow_forward
Sample Experimental Values:
Reaction 1: Both reactants are 2M
Reaction 2: Both Reactants are 2M
NaOH (aq) + HCl (aq) → H₂0 (1) + NaCl (39)
1
Reaction
2
NaOH (aq) + CH3COOH (aq) → H₂O (1) + NaCH3COO (ag)
Temperature Change
20 C
8 C
Volume of Reactants
25.0 mL NaOH
25.0 mL HCI
10.0 mL NaOH
10.0 mL CH3COOH
Final Mass of
Solution
50.0 g
20.0 g
arrow_forward
000
Lab Data
Welcome to Student Portal x
arrow_forward
Table 1: Gas Collection Data for Mg and HCI Reaction
Mass Mg (g)
0.040 g
Volume HC1 (mL)
10.00 mL
Concentration HC1
1.00 mol/L
(mol/L)
Atmospheric Pressure
14.50 psi
C
Temp Air (°C)
21.0
Temp Water (°C)
22.5
Volume of Gas (mL)
17.20
arrow_forward
●●●
6
15
16
Keynote File Edit Insert Slide Format Arrange View Play
...
17
18
19
20
21
✓
View
100%
Zoom
:0
F1
+
Add Slide
V
View
125%
Zoom
►
Play
+
Add Page
Keynote Live
F2
O
38,742
Table
20
T
Insert
F3
Share Window Help
APR
13
000
000
6
Table
GAS LAWS HOMEWORK ASSIGNMENT
(You can examine the data on the Student Data Sheets for assistance.)
F4
GASES LAB HW (1) ~
GASES LAB
Chart
.
Chart
T
Text
1.The pressure of a gas is doubled. Assuming that n and T are constant, what should
happen to the volume of the gas?
T
Text
2.The pressure of a gas is doubled. Assuming that n and V are constant, what should
happen to the temperature of the gas?
Shape
3.The number of moles of gas is doubled. Assuming P and T are constant, what should
happen to the volume of the gas?
F5
P
Media
Shape
density
PA
Media
Comment
F6
MacBook Air
◄◄
Comment
F7
No
Collaborate
Color Fill
Appearance
Title
Body
[Slide Number
▾ Background
▶11
4
Collab
F8
●
For
Sli
Edit M
arrow_forward
When nitroglycerine (227.1 g/mol) explodes, N₂, CO₂, H₂O, and O₂
gases are released initially. Assume that the gases from the explosion are
allowed to change to STP without reacting further.
4C₂H₂N₂O,(s)-6N₂(g) + 12 CO₂(g) + 10 H₂O(g) + O₂(g)
a. If 16.7 mol of nitroglycerine reacts, how many liters of nitrogen are
produced?
b. What is the total volume of gas produced when 1.000 kg of
nitroglycerine reacts?
arrow_forward
Purpose: The purpose of this lab is to determine the percent yield of hydrogen gas produced in the
reaction of magnesium solid with hydrochloric acid under conditions of Standard Temperature and
Pressure (STP).
Directions: Begin by printing out the Generating Hydrogen Lab (pdf file) posted below, and read
the introduction. Please watch the videos posted below, which will show you how the experiment
was done and also explain the calculations needed in this lab exercise. The video explaining the
calculations uses the data given in the lab manual, not the actual data from performing the
experiments. Make sure to use the data given below as your data for trials 1 and 2.
TRIAL 1 (from the 3-part video):
Mass of Mg: 0.083 g
Volume of H2 in cylinder: 73.2 mL
Temperature of H2 gas: 298 K
Barometric Pressure: 761 torr
TRIAL 2:
Mass of Mg: 0.066 g
Volume of H2 in cylinder: 62.0 mL
Temperature of H2 gas: 295 K (note a different temperature here, so there will be a different vapor
pressure of…
arrow_forward
Complete the highlighted section D
arrow_forward
Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured,
and found to be 0,55 atm.
key
carbon
hydrogen
nitrogen
sulfur
oxygen
chlorine
Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 2 significant digits. You may assume each gas behaves as an
ideal gas.
gas
mole fraction
partial pressure
atm
N2
|| atm
arrow_forward
* Question Completion Status:
A Moving to another question will save this response.
Question 26
SHOW WORK
Given the following reaction:
CaC 2(s) + 2H 20 - C2H 2(g) + Ca(OH) 2(aq)
Assume that you place 1.85 g of calcium carbide in excess water and collect the acetylene gas over water. Calculate the maximum amount of gas that should be produced in grams
round answer to 3 decimal places omit trailing zeroes
The actual volume of acetylene and water vapor collected is 810 ml at 30.5°C with a pressure of 557.524 mmHg.
Calculate the actual amount of gas collected(in grams)
round answer to 3 decimal places omit trailing zeroes
The vapor pressure of water at 30.5°C is 32.35 mmHg.
Calculate the percent yield of acetylene.
round answer to 2 decimal places omit trailing zeros
A Moving to another question will save this response.
arrow_forward
Some N2 gas is mixed with some O2 gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured,
and found to be 0.130 kPa.
key
carbon
hydrogen
nitrogen
sulfur
oxygen
chlorine
Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an
ideal gas.
gas
mole fraction
partial pressure
☐ x10
N2
||]
☐ kPa
☑
02
☐
☐ kPa
arrow_forward
A cylinder is filled with 10.0 L of gas and a piston is put into it. The initial pressure of the gas is measured to be 286. kPa.
The piston is now pushed down, compressing the gas, until the gas has a final volume of 4.00 L. Calculate the final pressure of the gas. Round your answer to 3
significant digits.
piston
cylinder
gas
| kPa
x10
arrow_forward
Please answer
arrow_forward
Please show how you got your answer. Thanks
arrow_forward
12.
(c) Potassium metal reacts with water.
2K(s)
+ 2H,0(1) → 2KOH(aq)
+ H,(g)
0.2346g of potassium is reacted with excess water.
Calculate the volume of gas formed.
The gas volume is measured in cm° at room temperature and pressure.
answer =
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
Related Questions
- Hi! I am unsure of how to solve this problem. Thank you!arrow_forwardneed help with qurstionarrow_forward2.) It’s a bad day in the lab! Two students are doing experiments. Each is 20 feet away from the professor. At the same time, each of them lets the same amount of a smelly gas into the room. One of them releases ammonia, NH3, and the other releases SO2. NH3 has a pungent odor, and SO2 smells like rotten eggs. The professor has no idea that this has happened, until she smell the first gas. Which chemical will the professor smell first? (NH3 or SO2) . If the professor starts to smell the first gas 42. seconds after the gas is released, how long will it take her to smell the second gas? sec. * Note: It is unsafe practice to work with these chemicals in an open lab.arrow_forward
- Only typed solution.arrow_forwardConsider the general chemical equation: 2A+2B-->4C+D. Part A. How many moles of C are produced from 2 mol of A? Express your answer as an integer and include appropriate units. Part B. How many porters of gas B must react to give 1L of gas D at the same temperature and pressure? express your answer as integer and include appropriate units.arrow_forwardearson.com/?courseld=1 ← 2 S MISSED THIS? Read Section 4.2 (Page); Watch KCV 4.2, IWE 4.2. W Write a balanced chemical equation for each reaction. म X → #3 E D C C $ 4 R F V % 5 T G B ^ ▾ 6 Part A G Search or type URL Y Aqueous hydrogen chloride reacts with oxygen gas to form chlorine gas and liquid water. Express your answer as a chemical equation. Identify all of the phases in your answer. ² ΑΣΦ H Submit Part B A chemical reaction does not occur for this question. Part C Request Answer Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water. Express your answer as a chemical equation. Identify all of the phases in your answer. Submit Request Answer MacBook Pro ΑΣΦ 4 A chemical reaction does not occur for this question. & 7 N Nitrogen monoxide gas reacts with hydrogen gas to form ammonia gas and water vapor. Express your answer as a chemical equation. Identify all of the phases in your answer. U J ☆ * 00 B 8 M C w ? I ? K ( 9. < O ) - O L P A I' Review I…arrow_forward
- hydroch 2. Unlike oxygen gas, nitrogen gas (the other major component of air) is generally unreactive. Magnesium is one metal that can react with nitrogen directly. What volume of nitrogen gas, measured at a pressure of 1.00 atm and a temperature of 27°C, will react with 5.0 g of magnesium? Mg(s) + N2(g) → Mg3N2(s). [unbalanced equation] cas and hyd what mass of ammon mitroge must decompose toarrow_forward江苏高考分数线 A Acellus Applications of the Ideal Gas Law 0.0453 moles of hydrogen gas were produced by the reaction. Calculate the volume of the gas at standard temperature and pressure. Mg + 2HCI → MgCl2 + H₂ Volume H₂ = [?]L C Liters of H₂ Enter 28 2 Resources Helparrow_forwardSample Experimental Values: Reaction 1: Both reactants are 2M Reaction 2: Both Reactants are 2M NaOH (aq) + HCl (aq) → H₂0 (1) + NaCl (39) 1 Reaction 2 NaOH (aq) + CH3COOH (aq) → H₂O (1) + NaCH3COO (ag) Temperature Change 20 C 8 C Volume of Reactants 25.0 mL NaOH 25.0 mL HCI 10.0 mL NaOH 10.0 mL CH3COOH Final Mass of Solution 50.0 g 20.0 garrow_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 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