Question

The Ideal Gas Law and Stoichiometry

The industrial production of nitric acid (HNO3) is a multistep process. The first step is the oxidation of ammonia (NH3) over a catalyst with excess oxygen (O2) to produce nitrogen monoxide (NO) gas as shown by the unbalanced equation given here:

?NH3(g)+?O2(g)→?NO(g)+?H2O(g)

Part A

What volume of O2 at 836 mmHg and 27 ∘C is required to synthesize 10.5 mol of NO?

Express your answer to three significant figures and include the appropriate units.

Answer 1

Balanced chemical reaction is

4NH_3(g)  + 5O_2(g)  → 4NO_(g) + 6H₂O_(g)

According to reaction to produce 4 mole of NO require 5 mole of O₂ then to produce 10.5 mole of NO required O₂=

10.5 X 5 / 4 = 13.125 mole of O₂ required

use ideal gas of equation to calculate volume of O₂ required

We know that PV = nRT

V = nRT/P

n = 13.125 mole,

T = 27⁰C = 27+273.15 = 300.15K,

P= 836 mmHg = 1.1 atm

R = 0.08205 L atm mol^-1 K^-1 ( R = gas constant)

V = ?

Substitute these value in above equation.

V = 13.125 X 0.08205 X300.15/ 1.1 = 293.85 L

293.85 liter O₂ required to produce 10.5 mole of NO