Question

Hi plz answer, i stupid 4.35 L of N2, at 25 ∘C and 1.16 atm , is mixed with 2.20 L of O2, at 25 ∘C and 0.277 atm , and the mixture allowed to react. N2(g)+O2(g)→2NO(g)

How much NO, in grams, is produced?

Answer 1

Mass = 1.5 g

Step-by-step explanation:

Given data:

Volume of N₂ = 4.35 L

Temperature = 25°C(25+273 = 298)

Pressure = 1.16 atm

Volume of O₂ = 2.20 L

Temperature = 25°C (25+273 = 298)

Pressure = 0.277 atm

Mass of NO produced = ?

Solution:

Chemical equation:

N₂ + O₂ → 2NO

Number of moles of N₂:

PV = nRT

n = PV/RT

n = 1.16 atm × 4.35 L / 0.0821 atm. L.K⁻¹. mol⁻¹×298 K

n = 5.046 atm. L/ 24.5 atm. L. mol⁻¹

n = 0.206 mol

Number of moles of O₂:

PV = nRT

n = PV/RT

n = 0.277 atm × 2.20 L / 0.0821 atm. L.K⁻¹. mol⁻¹×298 K

n = 0.609 atm. L/ 24.5 atm. L. mol⁻¹

n = 0.025 mol

Now we will compare the moles of NO with oxygen and nitrogen.

O₂ : NO

1 : 2

0.025 : 2×0.025=0.05 mol

N₂ : NO

1 : 2

0.206 : 2×0.206=0.412 moL

Number of moles of NO produced by oxygen are less so it will limiting reactant.

Mass of NO:

Number of moles = mass/molar mass

Mass = Number of moles × molar mass

Mass = 0.05 mol × 30 g/mol

Mass = 1.5 g