4 C3H5N3O9(l) + 6 N2(g) -> 12 CO2(g) + 10 H2O(g) + 1 O2(g) a. If 2.00 x 102 g worth of nitroglycerin (C3H5N3O9) completely decomposes, what is the total pressure of the gases created if they are collected in a 2.00 L container at 300.5 Celcius? b. If the total pressure of the mixture was actually 32.05 atm, calculate the partial pressures for each gas in the reaction
4 C3H5N3O9(l) + 6 N2(g) -> 12 CO2(g) + 10 H2O(g) + 1 O2(g) a. If 2.00 x 102 g worth of nitroglycerin (C3H5N3O9) completely decomposes, what is the total pressure of the gases created if they are collected in a 2.00 L container at 300.5 Celcius? b. If the total pressure of the mixture was actually 32.05 atm, calculate the partial pressures for each gas in the reaction
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter5: Gases
Section: Chapter Questions
Problem 5.99PAE: 99 Pure gaseous nitrogen dioxide (NO2) cannot be obtained, because NO2dimerizes, or combines with...
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4 C3H5N3O9(l) + 6 N2(g) -> 12 CO2(g) + 10 H2O(g) + 1 O2(g)
a. If 2.00 x 102 g worth of nitroglycerin (C3H5N3O9) completely decomposes, what is the total pressure of the gases created if they are collected in a 2.00 L container at 300.5 Celcius?
b. If the total pressure of the mixture was actually 32.05 atm, calculate the partial pressures for each gas in the reaction
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