At a certain temperature, the equilibrium constant for the following chemical equation is 3.50.
SO2(g) NO2(g) <--> SO3(g) NO(g)
At this temperature, calculate the number of moles of NO2(g) that must be added to 2.64 mol of SO2(g) in order to form 1.10 mol of SO3(g) at equilibrium.
Step-by-step? I cant figure it out.thnx
At a certain temperature, the equilibrium constant for the following chemical equation is 3.50. At this temper?
2017-01-11 4:22 pm
回答 (2)
2017-01-11 4:40 pm
Let y mol be the number of moles of NO₂ added.
SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g) …… Kc = 3.50
As the number of moles of gaseous molecules on the both sides are equal,
Kc =[SO₃] [NO] / {[SO₃] [NO₂]} = n(SO₃) n(NO)/{n(SO₃) n(NO₂)}
Initial amounts:
nₒ(SO₂) = 2.64 mol
nₒ(NO₂) = y mol
nₒ(SO₃) = 0 mol
nₒ(NO) = 0 mol
At equilibrium, 1.10 mol of SO₃ is formed.
Equilibrium amounts:
n(SO₂) = (2.64 - 1.10) mol = 1.54 mol
n(NO₂) = (y - 1.10) mol
n(SO₃) = 1.10 mol
n(NO) = (0 + 1.10) mol = 1.10 mol
Kc = n(SO₃) n(NO)/{n(SO₃) n(NO₂)}
1.10² / {1.54 × (y - 1.10)} = 3.50
y - 1.10 = 1.10² / {1.54 × 3.50}
y - 1.10 = 0.22
y = 1.32
The number of moles of NO₂ added = 1.32 mol
SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g) …… Kc = 3.50
As the number of moles of gaseous molecules on the both sides are equal,
Kc =[SO₃] [NO] / {[SO₃] [NO₂]} = n(SO₃) n(NO)/{n(SO₃) n(NO₂)}
Initial amounts:
nₒ(SO₂) = 2.64 mol
nₒ(NO₂) = y mol
nₒ(SO₃) = 0 mol
nₒ(NO) = 0 mol
At equilibrium, 1.10 mol of SO₃ is formed.
Equilibrium amounts:
n(SO₂) = (2.64 - 1.10) mol = 1.54 mol
n(NO₂) = (y - 1.10) mol
n(SO₃) = 1.10 mol
n(NO) = (0 + 1.10) mol = 1.10 mol
Kc = n(SO₃) n(NO)/{n(SO₃) n(NO₂)}
1.10² / {1.54 × (y - 1.10)} = 3.50
y - 1.10 = 1.10² / {1.54 × 3.50}
y - 1.10 = 0.22
y = 1.32
The number of moles of NO₂ added = 1.32 mol
2017-01-11 4:26 pm
I can't answer that one
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