Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: petstar21 on October 24, 2009, 07:33:51 PM
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Nitroglycerin decomposes:
4 C3H5(NO3)3(s) --> 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g)
Calculate the total volume of the gases at 1.2 atm and 25°C from 2.3 102 g of nitroglycerin.
** I was able to solve this part and got 149.81L
**This is the part I was confused on:
What are the partial pressures of the gases under these conditions in atm?
PCO2
PH2O
PN2
PO2
How can I solve this? help please
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First, you may want to delete one of your posts - since you double posted and one of these will eventually be locked by a moderator.
Secondly, I am not sure how you solved the first part, but I do know that however you solved it, do the same thing except when you get to the actual gases of CO2, H2O, N2, and O2, use only the moles (or grams) for the gases but with P. So instead of finding the partial pressures of ALL the gases use just PCO2, PH2O... instead of the total of all four gases.
Hope this helps,
The Cancer Curer
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How do i delete it?
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First, you may want to delete one of your posts - since you double posted and one of these will eventually be locked by a moderator.
These were different questions.
Secondly, I am not sure how you solved the first part, but I do know that however you solved it, do the same thing except when you get to the actual gases of CO2, H2O, N2, and O2, use only the moles (or grams) for the gases but with P. So instead of finding the partial pressures of ALL the gases use just PCO2, PH2O... instead of the total of all four gases.
What does it mean 'use only the moles (or grams) for the gases but with P'?
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How do i delete it?
No need to, although you should read forum rules (http://www.chemicalforums.com/index.php?topic=33740.0).