Answer:
2 C₇H₅N₃O₆ + 10.5 O₂ → 14 CO₂ + 5 H₂O + 3 N₂
73.96 g
Explanation:
Trinitrotoluene (TNT), C₇H₅N₃O₆, combines explosively with O₂ to produce CO₂, H₂O, and N₂. The balanced equation is:
2 C₇H₅N₃O₆ + 10.5 O₂ → 14 CO₂ + 5 H₂O + 3 N₂
The molar mass of C₇H₅N₃O₆ is 227.13 g/mol and there are 2 moles in the balanced equation. Then, 2 × 227.13 g = 454.26 g participate in the reaction.
The molar mass of O₂ is 31.998 g/mol and there are 10.5 moles in the balanced equation. Then, 10.5 × 31.998 g = 335.98 g participate in the reaction.
The mass ratio of C₇H₅N₃O₆ to O₂ is 454.26 g:335.98 g. The mass of O₂ that reacts with 100.0 g of TNT is:
100.0 g C₇H₅N₃O₆ × (335.98 g O₂/454.26 g C₇H₅N₃O₆) = 73.96 g O₂
Answer:
We need 73.92 grams of O2 for each 100 grams TNT
Explanation:
Step 1: Data given
Trinitrotoluene (TNT) = C7H5N3O6
oxygen = O2
Molar mass of TNT = 227.13 g/mol
Step 2: The balanced equation
4 C7H5N3O6 + 21O2 → 28CO2 + 10H2O + 6N2
Step 3: Calculate moles of TNT
Moles TNT = mass TNT / molar mass TNT
Moles TNT = 100.0 grams / 227.13 g/mol
Moles TNT = 0.440 moles
Step 4: Calculate moles of O2
For 4 moles TNT we need 21 moles of O2 to produce 28 moles CO2, 10 moles H2O and 6 moles N2
For 0.440 moles TNT we need 21/4 * 0.440 = 2.31 moles O2
Step 5: Calculate mass of TNT
Mass O2 = moles O2 * molar mass O2
Mass O2 = 2.31 moles * 32 g/mol
Mass O2 = 73.92 grams
We need 73.92 grams of O2 for each 100 grams TNT
