Detonation of nitroglycerin proceeds as follows:
\(4 \mathrm{C}_{3} \mathrm{H}_{5} \mathrm{~N}_{3} \mathrm{O}_{9}(l) & \longrightarrow \\
12 \mathrm{CO}_{2}(g)+6 \mathrm{~N}_{2}(g)+\mathrm{O}_{2}(g)+10 \mathrm{H}_{2} \mathrm{O}(g)\)
(a) If a sample containing 2.00 mL of nitroglycerin (density = 1.592 g/mL) is detonated, how many moles of gas are produced?
(b) If each mole of gas occupies 55 L under the conditions of the explosion, how many liters of gas are produced?
(c) How many grams of \(\mathrm{N}_{2}\) are produced in the detonation?
Text Transcription:
4 C3H5N3O9(l) \longrightarrow 12 CO2(g) + 6 N2(g) + O2(g) + 10 H2O(g)
{N}_{2}
Step 1 of 5) Relating ∆E to Heat and Work As we noted in Section 5.1, a system may exchange energy with its surroundings in two general ways: as heat or as work. The internal energy of a system changes in magnitude as heat is added to or removed from the system or as work is done on or by the system. If we think of internal energy as the system’s bank account of energy, we see that deposits or withdrawals can be made in the form of either heat or work. Deposits increase the energy of the system (positive ∆E), whereas withdrawals decrease the energy of the system (negative ∆E). We can use these ideas to write a useful algebraic expression of the first law of thermodynamics. When a system undergoes any chemical or physical change, the accompanying change in internal energy, ∆E, is the sum of the heat added to or liberated from the system, q, and the work done on or by the system, w: ∆E = q + w
