Final answer:
The mass of nitrogen dioxide that would be produced from 0.451 grams of nitric oxide can be found by calculating moles of NO from its mass, using the stoichiometric 1:1 ratio between NO and NO2 to find moles of NO2, and subsequently converting moles to mass of NO2 using its molar mass.
Step-by-step explanation:
To find the mass of nitrogen dioxide produced from the complete reaction of 0.451 grams of nitric oxide, we first need to use stoichiometry based on the balanced chemical equation:
2NO(g) + O₂(g) → 2NO₂(g)
From the equation, we see that 2 moles of NO react with 1 mole of O₂ to produce 2 moles of NO₂. Therefore, there is a 1:1 mole ratio between NO and NO₂.
First, we calculate the number of moles of NO using its molar mass (M(NO) = 30 g/mol):
Moles of NO = mass of NO / molar mass of NO = 0.451 g / 30 g/mol
Using the mole ratio from the balanced equation, we can now find the moles of NO₂ that would be produced. Since the ratio is 1:1, the moles of NO will be equal to the moles of NO₂. Next, we use the molar mass of NO₂ (M(NO₂) = 46 g/mol) to find the mass of NO₂ produced:
M(NO₂) = moles of NO₂ × molar mass of NO₂
After calculating these values, you would arrive at the mass of NO₂ in grams, which will match one of the multiple-choice options provided. Remember that all calculations should be performed to the correct number of significant figures from the given data and chemical molar masses.