Final answer:
To determine the mass of nitric oxide produced from 3.5g of ammonia, one must apply stoichiometry to a typical reaction where ammonia is oxidized to nitric oxide. Calculating the moles of ammonia and using the molar ratio from the balanced equation yields 6.17g of nitric oxide produced with the information given.
Step-by-step explanation:
The question asks what mass of nitric oxide is produced by the reaction of 3.5g of ammonia (NH3). To solve this, we need to consider the relevant chemical reaction and use stoichiometry to calculate the mass of nitric oxide produced. The provided information does not include a direct reaction for ammonia converting to nitric oxide, so we will assume a related typical reaction where ammonia is oxidized to produce nitric oxide (NO) like:
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
First, we need to calculate the number of moles of NH3:
Number of moles = mass (g) / molar mass (g/mol)
Ammonia has a molar mass of 17.031 g/mol, so:
Number of moles of NH3 = 3.5 g / 17.031 g/mol = 0.2055 mol
Using the stoichiometry of the reaction, for every 4 moles of NH3, 4 moles of NO are produced. Thus:
Moles of NO produced = 0.2055 mol (1 mol NO / 1 mol NH3)
Finally, we use the molar mass of NO (30.01 g/mol) to find the mass of NO produced:
Mass of NO = moles of NO * molar mass of NO
Mass of NO = 0.2055 mol * 30.01 g/mol = 6.1666 g
Therefore, 6.17 g of nitric oxide is produced from the reaction of 3.5 g of ammonia, with the result rounded to three significant figures in accordance with the information given.