How do we represent the decompositon of #C_3H_5(NO_3)_3#? And if #25.0*g# carbon dioxide were collected, what was the starting mass of the nitrate?

1 Answer
Feb 21, 2017

Answer:

A little too MANY grams for my liking..........

Explanation:

#4C_3H_5(NO_3)_3(l) rarr 12CO_2(g) + 6N_2(g) +10H_2O(g)+O_2(g)#

Is this balanced? How do you know? How is energy transferred during this reaction?

#"Moles of carbon dioxide"=(25.0*g)/(44.0*g*mol^-1)~=0.5*mol#

Given the stoichiometry, if there #0.5*mol# carbon dioxide are produced, then #0.167*mol# of the nitrate were consumed.

This represents a mass of,

#0.167*molxx227.09*g*mol^-1~=38*g.#

Funnily enuff, now the major use for this substance is probably as a medication in heart stimulants, and not for munitions and explosives. It's not chemistry that I'd like to do personally.