I would really appreciate it if someone would please help me out with this lab, Stoichiometry by Loss of CO2,

from my 12th grade chemistry class.

1. This experiment requires you to do 7 trials with varying amounts of Na2CO2.

2. Take a clean 50 mL beaker from the Glassware shelf and place it on the workbench. This is beaker # 1.

3. Take a balance from the Tools shelf and drop it on the beaker. Record the mass of the empty beaker.

4. Add 20 mL of 3M H2SO4 to the beaker. Measure and record the mass of the beakers again.

5. Add Na2CO2 to each beaker in the following amounts:

(a) To the first beaker, add 1g Na2CO2.

(b) To the second beaker, add 2g Na2CO2.

(c) To the third beaker, add 4g Na2CO2.

(d) To the fourth beaker, add 6g Na2CO2.

(e) To the fifth beaker, add 8g Na2CO2.

(f) To the sixth beaker, add 10g Na2CO2.

(g) To the seventh beaker, add 12g Na2CO2.

6. Bubbling of the CO2 gas indicates that a reaction has taken place. Weigh and record the mass of the beaker and its contents now.

7. Click on the beaker and drag it to the recycle bin on the right side of the workbench. Click ?Yes? to recycle the beaker and its contents.

8. Repeat Steps 3-6 with a second, third, fourth, fifth, sixth and seventh beaker. Drag the balance onto the new beaker to measure its mass. Make sure that you use the right amount of Na2CO2 for each beaker as indicated in Step 5!

Questions:
1. Record the amount of CO2 produced versus the amount of Na2CO2 used in each of the 7 beakers.

2.Discuss your results in terms of moles. Is there a linear relationship between the amoung of Na2CO2 used and the amount of CO2 produced?

Thank you for any assistance you can offer.
Tony

See the response by Dr Russ above.

To record the amount of CO2 produced versus the amount of Na2CO2 used in each of the 7 beakers, you will need to calculate the change in mass of each beaker before and after the reaction. Here's how you can do it:

1. Start with the mass of the empty beaker (recorded in Step 3) and subtract it from the mass of the beaker with the Na2CO2 (recorded in Step 6).

2. The difference in mass represents the mass of CO2 produced in each trial.

3. Repeat this calculation for each of the 7 beakers, using their respective masses recorded in Step 6.

4. Record the amount of CO2 produced in each trial.

Now let's move on to the second question:

To discuss your results in terms of moles and determine if there is a linear relationship between the amount of Na2CO2 used and the amount of CO2 produced, you need to convert the mass of CO2 produced to moles.

1. To convert mass to moles, you need to know the molar mass of CO2. The molar mass of CO2 is 44.01 g/mol.

2. Divide the mass of CO2 (in grams) produced in each trial by the molar mass of CO2 to get the number of moles.

3. Repeat this calculation for each trial, using the respective mass of CO2 produced.

4. Once you have the number of moles of CO2 produced in each trial, compare it to the amount of Na2CO2 used in each beaker.

If there is a linear relationship between the amount of Na2CO2 used and the amount of CO2 produced, you should observe that twice the amount of Na2CO2 used leads to twice the amount of CO2 produced, three times the amount of Na2CO2 used leads to three times the amount of CO2 produced, and so on.

I hope this helps you complete your lab. Good luck!