Question

C3H5N3O9(s) --> N2(g) + CO2(g) + H2O(g) + O2(g) Solid nitroglycerine explodes when heated, producing several different gases (according to the reaction above). If a government scientist explodes 777 g of nitroglycerine, How many grams of each gas should be produced? How many molecules of each gas will be produced?

Answer 1

- 143.6 g of N₂ ; 3.08×10²⁴ molecules of N₂

- 451.4 g of CO₂ ; 6.17×10²⁴ molecules of CO₂

- 153.9 g of H₂O ; 5.14×10²⁴ molecules of H₂O

- 27.3 g of O₂ ; 5.14×10²³ molecules of O₂

Step-by-step explanation:

This is a reaction of decomposition:

4C₃H₅N₃O₉(s) → 6N₂(g) + 12CO₂(g) + 10H₂O(g) + O₂(g)

4 moles of solid nitroglycerine decompose to 6 moles of nitrogen, 12 moles of carbon dioxide, 10 moles of water vapor and 1 mol of oxygen

We convert mass to moles → 777 g. 1mol/ 227g = 3.42 moles

4 moles of C₃H₅N₃O₉ can decompose to:

6 moles of N₂ ____ 12 moles of CO₂ ___ 10 moles of H₂O ___ 1 mol of O₂

Then, 3.42 moles of C₃H₅N₃O₉ may decompose to:

(3.42 . 6) / 4 = 5.13 moles of N₂

(3.42 . 12) / 4 = 10.26 moles of CO₂

(3.42 . 10) / 4 = 8.55 moles of water vapor

(3.42 . 1) / 4 = 0.855 moles of oxygen

We convert the moles to mass:

5.13 mol . 28 g/mol = 143.6 g of N₂

10.26 mol . 44 g/mol = 451.4 g of CO₂

8.55 mol . 18 g/mol = 153.9 g of H₂O

0.855 mol . 28 g/mol = 27.3 g of O₂

We count the atoms:

5.13 mol . 6.02×10²³ molecules /mol = 3.08×10²⁴ molecules of N₂

10.26 mol . 6.02×10²³ molecules /mol = 6.17×10²⁴ molecules of CO₂

8.55 mol . 6.02×10²³ molecules /mol = 5.14×10²⁴ molecules of H₂O

0.855 mol . 6.02×10²³ molecules /mol = 5.14×10²³ molecules of O₂