Your task is to produce 175mL of carbon dioxide. You many use anything in class.
Alright class. Your task is to produce 175mL of carbon dioxide. You many use anything in class. You have 1 class period to produce your product. You can use as much sodium carbonate and 1.0M hydrochloric acid as needed. ( Remember is stoichiometry lab)
Na2CO3 + 2HCl ==> H2O + CO2 + 2NaCl
You want 175 mL CO2. You know pressure and temperature of the lab. Use PV = nRT to calculate moles in 175mL CO2 at the conditions of the lab.
Using the coefficients in the balanced equation, convert moles CO2 desired to moles HCl.
Then using M = mols/L, solve for L of 1 M HCl needed.
Use the same process to determine mols Na2CO3, then convert moles Na2CO3 to grams. g = mols x molar mass.
You will need to work out the collection procedure, the lab set up, and that kind of thing.
Thank you so much!!! We do not know the pressure or temperature of the classroom though. This assignment was given to us for homework. We are to figure out the numbers and send them to our teacher then use them to do the lab in class tomorrow. Should we use a temp and pressure previously recorded in another lab?
To produce 175mL of carbon dioxide, you can follow these steps using materials commonly found in a classroom:
1. First, you need to identify a carbon source. One commonly available source in the classroom is a tablet of an antacid like calcium carbonate (CaCO3), which contains carbon.
2. Crush the antacid tablet into a fine powder using a mortar and pestle or any other suitable method.
3. Once you have the powdered antacid, transfer it to a test tube or any other small container that can withstand heat.
4. Now, you need to generate heat to facilitate the chemical reaction. If you have a Bunsen burner or a gas stove available in your classroom, you can use that. If an open flame is not allowed or not available, you can use an electric hot plate or even a candle.
5. Place the test tube, containing the powdered antacid, on a heat-resistant surface above the flame or hot plate. Ensure the opening of the test tube is directed away from yourself and others.
6. Apply heat to the test tube, gradually increasing the intensity, until the powdered antacid begins to react.
7. As the antacid reacts, it will release carbon dioxide gas (CO2). This gas will escape from the open end of the test tube.
8. To collect the generated carbon dioxide gas, you need a container that can trap gases, such as an inverted graduated cylinder or a gas collection tube submerged in water.
9. Insert the open end of the test tube into the container, making sure it is submerged in the water without letting any air escape.
10. As the reaction continues, the carbon dioxide gas will displace the water, causing it to rise and collect in the container. The volume of the collected gas will be measured in milliliters (mL).
11. Monitor the water level in the container until you have collected approximately 175mL of carbon dioxide gas.
12. Once you have collected the desired volume of carbon dioxide, remove the test tube from the heat source, carefully detach it from the gas collection container, and safely dispose of the remaining materials.
Please note that the reaction mentioned above is just one way to produce carbon dioxide gas in a classroom setting. Always ensure safety precautions are followed, such as proper ventilation, appropriate protective gear, and adherence to any specific guidelines or restrictions set by your teacher or school.