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------------------------------------------------ If [tex] 25.0 \mathrm{~g} [/tex] of [tex] \mathrm{NH}_{3} [/tex] and [tex] 38.6 \mathrm{~g} [/tex] of [tex] \mathrm{O}_{2} [/tex] react in the following reaction, what is the mass in grams of [tex] \mathrm{NO} [/tex] that will be formed?

Answer :

The mass of NO formed is 44.1 grams.

Mass of NH3 = 25.0 g

Mass of O2 = 38.6 g

We need to find the mass of NO formed.

Balanced chemical reaction equation:

[tex]4NH3 + 5O2 → 4NO + 6H2O[/tex]

Molecular weights:

NH3 = 14 + 3 = 17

O2 = 16 + 16 = 32

NO = 14 + 16 = 30

As per the balanced chemical reaction equation, 4 moles of NH3 reacts with 5 moles of O2 to produce 4 moles of NO and 6 moles of H2O.

Molar mass of NH3 = 17 g/mol

Molar mass of O2 = 32 g/mol

Molar mass of NO = 30 g/mol

Number of moles of NH3 = Mass / Molar mass

Number of moles of NH3 = 25.0 g / 17 g/mol

Number of moles of NH3 = 1.47 moles

Number of moles of O2 = Mass / Molar mass

Number of moles of O2 = 38.6 g / 32 g/mol

Number of moles of O2 = 1.21 moles

NH3 is the limiting reagent in this reaction as it produces fewer moles of NO, i.e., 1.47 moles.

NO formed from 1.47 moles of NH3 = 1.47 × 4/4 = 1.47 moles.

Mass of NO = Number of moles × Molar mass

Mass of NO = 1.47 moles × 30 g/mol

Mass of NO = 44.1 g

Therefore, 44.1 grams is the mass of NO formed.

To learn more about mass, refer below:

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