Nitroglycerin is a dangerous powerful explosive that violently decomposes when it is shaken or dropped. the swedish chemist alfred nobel (1833-1896) founded the nobel prizes with a fortune he made by inventing dynamite, a mixture of nitroglycerin and inert ingredients that was safe to handle. (1) write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin ( c3h5no33 ) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. (2) suppose 41.0l of carbon dioxide gas are produced by this reaction, at a temperature of −14.0°c and pressure of exactly 1atm . calculate the mass of nitroglycerin that must have reacted. round your answer to 3 significant digits.

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:

l dont know l am s sorry

the answer is 75.0%.