Question

Trinitrotoluene (TNT), C7H5N3O6, combines explosively with oxygen to produce CO2, water, and N2. Write a balanced chemical equation for the reaction and calculate the grams of oxygen required for each 100.0 g of TNT.

Answer 1

We need 73.92 grams of O2 for each 100 grams TNT

Step-by-step 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

Answer 2

2 C₇H₅N₃O₆ + 10.5 O₂ → 14 CO₂ + 5 H₂O + 3 N₂

73.96 g

Step-by-step 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