Question

Liquid nitroglycerin has a density of approximately 1.60 g/mL. The nitroglycerin decomposition reaction equation is:

4C3H5N3O9 (l)-+ 12 CO2 (g) → 10 H2O(g) + 6 N2(g) + О2 (g)

Assume that when heated to 218.0°C, 1.00 lb of nitroglycerin explodes heating the product gases to 750.0°C. Determine the total gas volume, in L, produced by the explosion.

Answer 1

Step-by-step explanation:

Density = 1.60 g/mL

Initial Temperature T1 = 218.0°C + 273 = 491 K (Upon converting to kelvin temperature)

Final Temperature T2 = 750.0°C + 273 = 1023 K (Upon converting to kelvin temperature)

Mass of gas = 1.00 lb = 453.592 g (Upon converting to g)

Final Volume V2 = ?

Initial volume can be obtained from;

Density = Mass / Volume

Volume = Mass / Density

Volume = 453.592 / 1.60 = 283.495 ml

Initial Volume V1 = 283.495 ml

Using charles law;

V1 / T1 = V2 / T2

V2 = V1 * T2 / T1

V2 = 283.495 * 1023 / 491

V2 = 590.66 ml