Answer:
10.54 L
Explanation:
Given that:-
Moles of
= 1.00 moles
According to the given reaction:-
![4NH_3+7O_2\rightarrow 4NO_2+6H_2O](https://tex.z-dn.net/?f=4NH_3%2B7O_2%5Crightarrow%204NO_2%2B6H_2O)
7 moles of oxygen gas reacts with 4 moles of ammonia
1 mole of oxygen gas reacts with
moles of ammonia
Moles of ammonia = 0.5714 moles
Also, Given that:
Temperature = 850 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (850 + 273.15) K = 1123.15 K
n = 0.5714 moles
P = 5.00 atm
Using ideal gas equation as:
![PV=nRT](https://tex.z-dn.net/?f=PV%3DnRT)
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L atm/ K mol
Applying the equation as:
5.00 atm × V = 0.5714 moles ×0.0821 L atm/ K mol × 1123.15 K
⇒V = 10.54 L
<u>10.54 L of
required.</u>