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?
thanks
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?
thanks
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
...1.00.......0.00943.......?.....0.00943
...2.00.......0.01887.......?.....0.01887
...3.00.......0.02830.......?.....0.02830
...4.00.......0.03772........?....0.0377
etc.
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.
To analyze the stoichiometry loss of CO2 in your experiment, you need to examine the relationship between the amount of Na2CO3 used and the amount of CO2 produced. Here's how you can approach it:
1. Record the amount of CO2 produced vs the amount of Na2CO3:
In your experiment, you conducted 7 trials using 20ml of 3M H2SO4 and added varying amounts of Na2CO3 to each. Make sure to document the precise amounts of Na2CO3 used for each trial, as well as the corresponding CO2 produced. This data will help you determine whether there is a relationship between the two variables.
2. Convert the measured amounts of Na2CO3 and CO2 into moles:
To analyze the relationship between Na2CO3 and CO2 in terms of moles, you need to convert the measured amounts of Na2CO3 and CO2 into moles. This can be done using the molar mass of each compound. The molar mass of Na2CO3 can be calculated by adding up the atomic masses of the elements in the compound (2 sodium atoms, 1 carbon atom, and 3 oxygen atoms). The molar mass of CO2 is the sum of the atomic masses of 1 carbon atom and 2 oxygen atoms.
3. Plot the moles of Na2CO3 (x-axis) against the moles of CO2 (y-axis):
Once you have determined the moles of Na2CO3 and CO2 for each trial, plot the data on a graph. Place the moles of Na2CO3 on the x-axis and the moles of CO2 on the y-axis. This will allow you to visualize the relationship between the two variables.
4. Analyze the plotted data:
Examine the graph to determine whether there is a linear relationship between the amount of Na2CO3 used and the amount of CO2 produced. If the graph shows a straight line passing through the origin (0,0), it suggests a direct proportionality. This would indicate a consistent stoichiometry loss of CO2 based on the amount of Na2CO3 used.
However, if the graph deviates from a straight line or does not pass through the origin, it suggests a non-linear relationship or deviations from stoichiometry. In such cases, additional factors might be influencing the CO2 production, such as incomplete reaction, side reactions, or other variables.
By following these steps, you can analyze the stoichiometry loss of CO2 in your experiment and determine whether there is a linear relationship between the amount of Na2CO3 used and the amount of CO2 produced.