posted by janey on .
i have 2 questions
stoichiometry loss of CO2
1. record the amount of CO2 produced vs the amount of Na2CO3. I did 7 beakers with 20ml of 3M H2SO4 and add varying amounts of Na2CO3 to each.
2. discuss your results in terms of moles. is there a linear relationship between the amount of Na2CO3 used and the amount of CO2 produced?
A paucity of information.
i was given an equation of
H2SO4(1)+ Na2CO3(s)>>> Na2SO4(s)+CO2(g)+H2O(l)
I tried plugging in numbers and I don't understand what I am supposed to do.
the first beaker had 1g of Na2CO3 and added 20ml of 3M H2SO4 to the beaker.
empty beaker 47.42g
beaker with 1g and 20ml added 70.62g
(s) before 48.420
can you get me started on this and did I give enough info yet?
From the two posts I'm guessing you started with 7 beakers with 20 mL of 3M H2SO4 and you weighed those. Then you added 1 g Na2CO3 to the first one, 2g to the second one, 3 g to the third one, etc.After the reaction, I assume you weighed the beakers again.
How did you measure the CO2? Did you measure it by volume or by loss in weight? Probably by loss in weight.
Convert g Na2CO3 to moles. moles = grams/molar mass
Convert g CO2 to moles. g/molar mass = moles.
Then try plotting the data.
You might try g Na2CO3 vs g CO2 for one plot.
You might try moles Na2CO3 vs moles CO2 for another one. The problem sounds as if this is what they want. You should get a 1:1 relationship since 1 mole Na2CO3 produces 1 mole CO2 according to the equation Na2CO3 + H2SO4 ==> Na2CO3 + H2O + CO2.
I've had some time to think about this and I think you can make it simpler. Make a table something like this.
...g Na2CO3...mol Na2CO3...g CO2...mol CO2
You may not have used exactly 1.00, 2.00 g Na2CO3. Use in the table the amount you weighed.
moles Na2CO3 = grams/106
moles CO2 = grams/44
moles Na2CO3 column should equal moles in the CO2 column.