Combustion Problem

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Andrea- 3J
Posts: 56
Joined: Tue Nov 14, 2017 3:00 am

Combustion Problem

Postby Andrea- 3J » Fri Oct 19, 2018 11:49 pm

"Salicylic acid is the precursor to the active ingredient in aspirin and was used in history as an early painkiller. It has the formula C7H6O3. If you took a 1.35g pill containing 15% salicylic acid by weight, how many grams of carbon dioxide would you exhale as a result of digesting the salicylic acid?"
I need help understanding how to start this problem and using the information it gave us.



The balanced equation is C7H6O3 + 7O2 ->7CO2 + 3H2O

505211599
Posts: 60
Joined: Fri Sep 28, 2018 12:28 am

Re: Combustion Problem

Postby 505211599 » Sat Oct 20, 2018 12:58 am

To start the problem, you would first calculate how many grams of salicylic acid is contained in the pill. You would do this by multiplying the 1.35g by 0.15. Keep in mind that because this is a percent, the number of significant figures would still be 3. You would then convert the grams of salicylic acid to moles of salicylic by dividing the grams of salicylic acid by the molar mass of salicylic acid. Then you would use stoichiometric calculations to find the grams of CO2 exhaled.


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