2.7: Gas Laws-Simulations and Wet Lab-Home
- Page ID
- 387435
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- To experiment with variables to reach gas law relationships
- To verify Avogadro's law
- To improve problem-solving skills by practicing gas-law problems
Theory
If you observe a parameter (dependent variable), say volume by changing any one of the other parameters (independent variable) like pressure, (keep the rest at constant of fixed value) you may come across some kind of data trends regarding the dependence of volume on increasing or decreasing the pressure. If you follow the results of such experiments by systematic observation and analysis you can hypothesize the relationship between the parameters. You can repeat the same experiment many times. If the trend is generalizable it could be stated as a LAW. This is how many science laws are postulated, including the simple gas laws. There are three simple gas laws studying the various parameters like temperature (T), pressure (P), and number of moles of gas particles (n) on the volume (V) of a gas. Following are the laws and the parameters they correlate
· Boyle’s Law (relates Volume and Pressure: V and P)
· Charles Law (relates Volume and Temperature: V and T)
· Avogadro’s Law (relates Volume and Number of particles: V and n)
In PART A of the experiment a free online simulation on all the four parameters (V, T, P, and n) will be accessed to play around with the parameters to see how they are related, and to predict the trend in the results.
In PART B of the experiment a gas evolution reaction will be followed to observe the effect of adding more particles (n) on the volume (V) of the gas to postulate the Avogadro’s law. A graphical analysis of the data will also be done.
Procedure
Materials Required
A laptop to play the gas law simulation online, Five (16 Fl. Oz) empty water or cola bottles with narrow mouth (any type of bottles of the same size and shape with narrow mouth). Five to six medium sized balloons. Baking soda (Sodium bicarbonate), 5% Vinegar (acetic acid), spoons, 5-cups, funnel (or a paper cone to bes used as a funnel to transfer the powder to the balloon, electronic scale, graduated cylinders, water
Part A: Simulations to Verify Simple Gas Laws and Ideal Gas Law
The major difference between solid, liquid, and gas phases is how the particles in a phase are packed. Component particles in a gas are widely separated as if there is no interaction between them. Because of this reason, a gas can be compressed further and further down to smaller volumes (space). Most of the gases are colorless. Therefore, it is very difficult to observe them for experimental purposes. However, some parameters of gases are measurable like their volume, pressure, temperature, and number (moles) of particles present.
- Turn on your lap top. Access the internet and the go to the free online gas simulation website provided by your instructor
- Connect to the webpage, and play around with the simulation by changing volume, pressure, temperature and number of molecules by clicking and dragging the various bars after selecting one.
Boyle’s law
- Click on the pressure button on the drag and drop bar on the right hand side. Keep the number of moles (n) and Temperature fixed at constant values. Record them. Now go ahead and drag the button on pressure bar and leave at any five different values and observe the volume reading. Record five different pressure values and the corresponding volumes on the observation sheet. This can be used to predict the relationship between the pressure and volume. This relationship is the concept behind the Boyle’s law.
Charle’s law
- Click on the volume button on the drag and drop bar on the right hand side. Keep the number of moles (n) and Pressure fixed at constant values. Write them down. Now go ahead and drag the button on temperature (T) bar and leave at any five different values and observe the volume reading. Record all the five different Temperature values and the corresponding volumes on the observation sheet. This can be used to predict the relationship between the temperature and volume. This relationship is the concept behind the Charle’s law.
Ideal gas law
- Click on the volume button on drag and drop bar on the right hand side. Play around with the temperature (T) and Pressure at various values. Now go ahead and . Record all the five different corresponding sets of Volume, Pressure, and Temperature values. Calculate the number of moles using the ideal gas equation. The value of Ideal gas constant, R should be taken as 0.08206 L.atm/mol.K.
Part B: Wet Lab to Test Avogadro's Law
Watch the following Youtube video. We will se up a similar experiment.
Instead of the conical flask we will be using five identical water or cola bottles (16 Fl. Oz). Also, we will have a total of five sample instead of the four shown in the solution. The acetic acid we have is the 5% vinegar. 5% vinegar is approximately 0.83M not 1.0M as shown in the video. In order to get 0.19 mol of acetic acid in each bottle, you need to take 229 ml of the 5% (0.83M).
- Use the M1V1=M2V2 equation to find out the new volume 1.0 M x 190 ml =0.83 M x X ml. On solving for X you will get 229 ml as the new volume.
- Take five medium size water or cola bottles of the same size and shape (16 Fl. Oz). Label them as 3, 7, 12, 16, and 20 using a marker.
- Measure out 229 ml of 0.83M acetic (5% vinegar) into each bottle.
- Measure 3 g, 7 g, 12 g, 16 g, 20 g sodium bicarbonate (NaHCO3) or baking soda separately in small containers.
- Without spilling add the powder into five similar sized balloons using a funnel, and keep them aside.
- Align each balloon by the side of each bottle. The balloons should be attached on the mouth of the bottles tightly while taking care not to spill the powder into the flask. Hold the balloons tight as shown in the video, as it might fly off as large amount of gas is produced.
- Once all the balloons are attached tightly, all the balloons should be flipped to release the powder into the bottle as shown in the video.
- Record the observation on the report sheet. Take a lab picture
- Compare the volume of the balloons with the amount of the gas particles produced. Observe the trend in the volume and enter it in the observation sheet.
- Following is the reaction between the acetic acid and sodium bicarbonate producing water, sodium acetate, and carbon dioxide gas. Analyze the relationship between the volume and number of moles of gas particles produced and state your hypothesis.
- Keep this observation and data sheet to reuse in the lab for Mole ratios and limiting reactant
Report Sheet
Part A: Simulations to Verify Simple Gas Laws and Ideal Gas Law
Boyle's Law
|
Constant Temperature= K Constant number of moles = mol |
||
| # | Pressure ( Atm) | Volume (L) |
| 1 | ||
| 2 | ||
| 3 | ||
| 4 | ||
| 5 | ||
Charle' Law
|
Constant Pressure = Atm Constant number of moles = mol |
||
| # | Temperature ( K) | Volume (L) |
| 1 | ||
| 2 | ||
| 3 | ||
| 4 | ||
| 5 | ||
Ideal Gas Law
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Calculate the number of mols, n for each set of data. Use the value of Ideal gas constant R as 0.08206 L.atm/mol.K |
||||
| # | P, Pressure ( Atm) | V, Volume (L) | T, Temperature (K) | ? mols (n) |
| 1 | ||||
| 2 | ||||
| 3 | ||||
| 4 | ||||
| 5 | ||||
Report Sheet: Part B-Wet Lab to Test Avogadro's Law
Avogadro's Law
|
Constant Temperature= K (Room temperature) Constant Pressure = 1.0 Atm |
||||
| # | Grams of Sodium bicarbonate used | Moles, n, of bicarbonate used | Moles of Carbon dioxide produced ( assume 1:1 mol ratio) | Rate the size of the inflated balloons on a scale of 1-4, 1 being the smallest |
| 1 | 3.0 g | mol | ||
| 2 | 7.0 g | mol | ||
| 3 | 12.0 g | mol | ||
| 4 | 16.0 g | mol | ||
| 5 (Do not use this data for this lab. Reserve this for the Moles and Limiting Reactant Lab) | 32.0 g | mol | ||
Data Analysis
1. On analyzing the data in Part A simulation for Boyle's law, how are the Volume and Pressure related? Write your statement. Does this match with the theoretical statement given at the beginning of the experiment?
2. On analyzing the data in Part A simulation for Charle's law, how are the Volume and Temperature related? Write your statement. Does this match with the theoretical statement given at the beginning of the experiment?
3. On analyzing the data in Part B for Avogadro's law, how are the Volume (size of the balloons) and the number of moles of the gas produced related? Write your statement. Does this match with the theoretical statement given at the beginning of the experiment?
4. On analyzing the data in Part A simulation for the Ideal gas law, how are the number of moles related? Are you getting similar values or very different values? Explain your findings
5. Plot a graph with your independent variable in Part A Boyle's law, pressure vs. volume. Give a proper title, and label the axes with the parameters and the units.
Practice Problems
If 3.7L of an ideal gas at 35.8 degree Celsius and 1.5atm is heated to 373.5 K, what would be the new pressure as the gas has expanded to 7.8 L?
- Answer
-
0.59 atm
Pick one of the entries from Part A-Ideal gas law simulation. Write the number of moles calculated in one of those five data points. Convert the number of moles to the mass of the gas assuming that the gas in the simulation is Carbon monoxide or CO.
- Answer
-
Clue: n mol=Mass (g)/Formula mass (g/mol). Therefore, Mass (g)= n mol X Formula mass (g/mol)
Contributions and Attributions
Manjusha Saraswathiamma, Minnesota State Community and Technical College, Moorhead has developed this experiment to conduct this at a homeschool setting using less hazardous and cost-effective materials. The author would like to acknowledge the creators (Ohio State University) of the Youtube video used in this experiment. A portion of the Theory part is a content reuse form Chem 10 Experiment Experimental Determination of the Gas Constant (Experiment) by Santa Monica College is licensed CC BY-NC 4.0.