Final answer:
To calculate the mass of nitric oxide from 6.82 g of NH₃, perform a stoichiometry based on the mole ratio from the balanced equation. First, find moles of NH₃, then use the 1:1 mole ratio with NO to find moles of NO, and finally calculate the mass of NO, yielding 12.03 g of NO produced.
Step-by-step explanation:
To determine the mass of nitric oxide (NO) produced from 6.82 g of ammonia (NH₃), we need to perform a stoichiometric calculation based on the balanced chemical equation 4NH₃ + 5O₂ → 4NO + 6H₂O. First, calculate the molar mass of NH₃ which is approximately 17 g/mol. Then, find the moles of NH₃ by dividing the given mass of NH₃ by its molar mass.
Next, use the stoichiometric coefficients from the balanced equation to establish the mole ratio between NH₃ and NO, which is 1:1. This means that the moles of NH₃ will be equal to the moles of NO produced. After finding the moles of NO, calculate the mass of NO by multiplying the moles of NO by the molar mass of NO, which is approximately 30 g/mol.
The calculation steps are as follows:
Calculate moles of NH₃: 6.82 g NH₃ ÷ 17 g/mol = 0.401 moles NH₃.
Determine moles of NO using the mole ratio: 0.401 moles NH₃ (1 mole NO / 1 mole NH₃) = 0.401 moles NO.
Calculate mass of NO: 0.401 moles NO × 30 g/mol = 12.03 g NO.
Therefore, 6.82 g of NH₃ can produce 12.03 g of nitric oxide.