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: 47.420g
4. Add 20 mL of 3M H2SO4 to the beaker. Measure and record the mass of the beakers again: 70.035g
5. Add Na2CO2 to each beaker in the following amounts:
(a) To the first beaker, add 1g Na2CO2. Total mass: 70.620g
(b) To the second beaker, add 2g Na2CO2. Total mass: 71.205g
(c) To the third beaker, add 4g Na2CO2. Total mass: 72.375g
(d) To the fourth beaker, add 6g Na2CO2. Total mass: 73.544g
(e) To the fifth beaker, add 8g Na2CO2. Total mass: 75.395g
(f) To the sixth beaker, add 10g Na2CO2. Total mass: 77.395g
(g) To the seventh beaker, add 12g Na2CO2. Total mass: 79.395g
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 amount of Na2CO2 used and the amount of CO2 produced?
Thank you for any assistance you can offer.
Tony
1. You will have results for this.
2. You need the correct formula which is Na2CO3. To decide if there is a linear relation ship plot the number of moles of CO2 produced (y-axis) against moles of Na2CO3 used (x-axis)
To calculate the number of moles this is mass/molar mass.
molar mass of CO2 = 44
I'll let you work out molar mass of Na2CO3
To answer your questions, we need to analyze the data and calculate the amount of CO2 produced in each beaker and the mole ratios between Na2CO2 and CO2.
Step 1:
Record the amounts of Na2CO2 used in each beaker from Step 5:
(a) 1g Na2CO2
(b) 2g Na2CO2
(c) 4g Na2CO2
(d) 6g Na2CO2
(e) 8g Na2CO2
(f) 10g Na2CO2
(g) 12g Na2CO2
Step 2:
Calculate the change in mass (mass of beaker and contents - mass of empty beaker) for each beaker in Step 6:
(a) Change in mass = 70.620g - 47.420g
(b) Change in mass = 71.205g - 47.420g
(c) Change in mass = 72.375g - 47.420g
(d) Change in mass = 73.544g - 47.420g
(e) Change in mass = 75.395g - 47.420g
(f) Change in mass = 77.395g - 47.420g
(g) Change in mass = 79.395g - 47.420g
Step 3:
Convert the change in mass to the amount of CO2 produced using the molar mass of CO2 (44.01 g/mol).
(a) Amount of CO2 produced = (Change in mass of beaker and contents)/(Molar mass of CO2)
(b) Amount of CO2 produced = (Change in mass of beaker and contents)/(Molar mass of CO2)
(c) Amount of CO2 produced = (Change in mass of beaker and contents)/(Molar mass of CO2)
(d) Amount of CO2 produced = (Change in mass of beaker and contents)/(Molar mass of CO2)
(e) Amount of CO2 produced = (Change in mass of beaker and contents)/(Molar mass of CO2)
(f) Amount of CO2 produced = (Change in mass of beaker and contents)/(Molar mass of CO2)
(g) Amount of CO2 produced = (Change in mass of beaker and contents)/(Molar mass of CO2)
Step 4:
Plot the amount of Na2CO2 used on the x-axis and the amount of CO2 produced on the y-axis.
Based on the plot, analyze the relationship between the two values and determine if it is linear or not. If the plot shows a straight line passing through the origin, it indicates a linear relationship between the amount of Na2CO2 used and the amount of CO2 produced.