For the equilibrium: 2 SO3(g) <=> 2 SO₂(g) + O₂(g) K₁ = Kc Calculate Ko at this temperature. Solution The reaction K value has been measured in concentration, thus is a Ke value. We need to change that to Kp. T = 1.00 x 10³ K Thus: = 4.08 x 10-3 at 1.00 x 10³ K. R = 0.08206 L-atm/mol K An = 3-2 = 1 Δη K₂ = K (RT) An => Kp K₂ (4.08 x 10-³)[(0.08206) (1000)] Kp = 0.335 =

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I did the calculation and I found 3.34 and would it be wrong if I put this as my answer

For the equilibrium: 2 SO3(g) <=> 2 SO₂(g) + O₂(g)
K₁ =
Kc
Calculate Ko at this temperature.
Solution
The reaction K value has been measured in concentration, thus is
a Ke value.
We need to change that to Kp.
T = 1.00 x 10³ K
Thus:
= 4.08 x 10-3 at 1.00 x 10³ K.
R = 0.08206 L-atm/mol K
An = 3-2 = 1
Δη
K₂ = K (RT) An =>
Kp
K₂ (4.08 x 10-³)[(0.08206) (1000)]
Kp = 0.335
=
Transcribed Image Text:For the equilibrium: 2 SO3(g) <=> 2 SO₂(g) + O₂(g) K₁ = Kc Calculate Ko at this temperature. Solution The reaction K value has been measured in concentration, thus is a Ke value. We need to change that to Kp. T = 1.00 x 10³ K Thus: = 4.08 x 10-3 at 1.00 x 10³ K. R = 0.08206 L-atm/mol K An = 3-2 = 1 Δη K₂ = K (RT) An => Kp K₂ (4.08 x 10-³)[(0.08206) (1000)] Kp = 0.335 =
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