Answer:
a.
b. 146.0 g
Explanation:
Question 1 (a). Just as the problem states, liquid nitroglycerin decomposes into nitrogen gas , oxygen gas
, water vapor
and carbon dioxide
. Let's write the decomposition of nitroglycerin into these 4 components:
Now we need to balance the equation. Firstly, notice we have 3 carbon atoms on the left and 1 on the right, so let's multiply carbon dioxide by 3:
Now, we have 3 nitrogen atoms on the left and 2 on the right, so let's multiply nitrogen on the right by :
We have 5 hydrogen atoms on the left, 2 on the right, so let's multiply the right-hand side by :
Finally, count the oxygen atoms. We have a total of 9 on the left. On the right we have (excluding oxygen molecule):
This leaves of oxygen. Since oxygen is diatomic, we need to take one fourth of it to get one half in total:
To make it look neater without fractional coefficients, multiply both sides by 4:
Question 2 (b). Now we can make use of the balanced chemical equation and apply it for the context of this separate problem. We're given the following variables:
Firstly, we may find moles of carbon dioxide produced using the ideal gas law .
Rearranging for moles, that is, dividing both sides by RT (here R is the ideal gas law constant):
According to the stoichiometry of the balanced chemical equation:
4 moles of nitroglycerin (ng) produce 12 moles of carbon dioxide. From here we can find moles o nitroglycerin knowing that:
Multiplying the number of moles of nitroglycerin by its molar mass will yield the mass of nitroglycerin decomposed: