Respuesta :
Answer:
13.05 gNO
Explanation:
60g NO2 x 1 mol NO2 / 46.01 gNO2 x 1 mol NO / 3 mol NO2 x 30.01 gNO / 1 mol NO = 13.05gNO
The mass of NO that would be produced from the reaction is 13.05 g
From the question,
We are to determine the mass of NO that would be produced.
The given balanced chemical equation for the reaction is
3NO₂(g) + H₂O(l) → 2HNO₃(g) + NO(g)
This means
3 moles of NO₂ reacts with 1 mole of H₂O to produce 2 moles of HNO₃ and 1 mole of NO
Now, we will determine the number of moles of NO₂ present
Mass of NO₂ = 60.0 g
Molar mass of NO₂ = 46.0055 g/mol
Using the formula
[tex]Number\ of\ moles =\frac{Mass}{Molar\ mass} \\[/tex]
∴ Number of moles of NO₂ present = [tex]\frac{60.0}{46.0055}[/tex]
Number of moles of NO₂ present = 1.3041919 moles
From the balanced chemical equation
3 moles of NO₂ reacts with H₂O to produce 1 mole of NO
Then,
1.3041919 moles of NO₂ reacts with excess H₂O to produce [tex]\frac{1.3041919}{3}[/tex] mole of NO
[tex]\frac{1.3041919}{3}[/tex] = 0.4347306 mole
∴ 0.4347306 mole of NO will be produced
Now, for the mass of NO that would be produced
From the formula
Mass = Number of moles × Molar mass
Molar mass of NO = 30.01 g/mol
∴ Mass of NO that would be produced = 0.4347306 × 30.01
Mass of NO that would be produced = 13.05 g
Hence, the mass of NO that would be produced from the reaction is 13.05 g
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