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Stoichiometry Problem: Gram to Gram The explosion of nitroglycerine is described by the equation:...

Stoichiometry Problem: Gram to Gram
The explosion of nitroglycerine is described by the equation:
4C3H5(NO3)3 -> 12CO2 + 10H2O + 6N2 + O2
How many grams of carbon dioxide is produced by the explosion of 21.0 g of nitroglycerine?

Answer

To solve this problem, we need to use stoichiometry to convert grams of nitroglycerine to grams of carbon dioxide.

  1. Calculate the molar mass of nitroglycerine (C3H5(NO3)3):
    • Carbon (C): 12.01 g/mol × 3 = 36.03 g/mol
    • Hydrogen (H): 1.01 g/mol × 5 = 5.05 g/mol
    • Nitrogen (N): 14.01 g/mol × 3 = 42.03 g/mol
    • Oxygen (O): 16.00 g/mol × 9 = 144.00 g/mol
    • Total molar mass = 36.03 + 5.05 + 42.03 + 144.00 = 227.11 g/mol
  2. Calculate the moles of nitroglycerine in 21.0 g:
    • Moles of nitroglycerine = 21.0 g / 227.11 g/mol = 0.0925 mol
  3. Use the stoichiometry of the reaction to find moles of CO2 produced:
    • From the equation, 4 moles of C3H5(NO3)3 produce 12 moles of CO2.
    • Moles of CO2 = 0.0925 mol C3H5(NO3)3 × (12 mol CO2 / 4 mol C3H5(NO3)3) = 0.2775 mol CO2
  4. Calculate the mass of CO2 produced:
    • Molar mass of CO2 = 12.01 + 16.00 × 2 = 44.01 g/mol
    • Mass of CO2 = 0.2775 mol × 44.01 g/mol = 12.21 g

Therefore, 12.21 grams of carbon dioxide are produced by the explosion of 21.0 g of nitroglycerine.

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