Answer:
Mass = 1.5 g
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
