5 moles each of SO₂ and O₂ are allowed to react in a one litre vessel. At equilibrium, moles of SO3 is found to be 3. Select the correct option(s) regarding the equilibrium. 2SO₂(g) + O₂(g) 2SO3(g) (A) Partial pressure of O₂ is 0.41 times of equilibrium pressure. (B) 60% of SO₂ is consumed to acquire equilibrium (C) 30% of O₂ is consumed to acquire equilibrium (D) All of these
Answers & Comments
Answer:
The reaction is depicted as:
S
O
2
+
1
2
O
2
⟷
S
O
3
We have initially:
S
O
2
=
5
mol
O
2
=
5
mol
S
O
3
=
0
mol
At equilibrium :
60%
S
O
2
is used up-
S
O
2
=
5
−
5
(
0.6
)
=
2
mol
O
2
=
5
−
5
(
0.3
)
=
3.5
mol
S
O
3
=
5
(
0.6
)
=
3
mol
Therefore, total moles of
S
O
2
,
O
2
and
S
O
3
at equilibrium
=
8.5
mol