Question

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?

Answer 1

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.