1. Write the Balanced Chemical Equation:
The reaction you're describing is the decomposition of nitrogen monoxide (NO) to form nitrogen dioxide (NO₂) and oxygen (O₂):
2NO(g) + O₂(g) → 2NO₂(g)
2. Determine the Mole Ratio:
From the balanced equation, we see that for every 2 moles of NO₂ produced, 1 mole of O₂ is produced.
3. Calculate the Moles of NO₂:
You need to convert the given amount of NO₂ (11.5 g) into moles using its molar mass.
* Molar mass of NO₂ = 14.01 g/mol (N) + 2 * 16.00 g/mol (O) = 46.01 g/mol
* Moles of NO₂ = (11.5 g NO₂) / (46.01 g/mol NO₂) = 0.25 moles NO₂
4. Calculate the Moles of O₂:
Using the mole ratio from the balanced equation:
* Moles of O₂ = (0.25 moles NO₂) * (1 mole O₂ / 2 moles NO₂) = 0.125 moles O₂
5. Convert Moles of O₂ to Grams:
* Molar mass of O₂ = 2 * 16.00 g/mol = 32.00 g/mol
* Grams of O₂ = (0.125 moles O₂) * (32.00 g/mol O₂) = 4.00 g O₂
Therefore, 4.00 grams of oxygen are produced when 11.5 grams of NO₂ is formed.
