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zvonat [6]
3 years ago
13

At T = 250 °C the reaction PCl5(g) PCl3(g) + Cl2(g) has an equilibrium constant in terms of pressures Kp = 2.15. (a) Suppose the

initial partial pressure of PCl5 is 0.548 atm, and PPCl3 = PCl2 = 0.780 atm. Calculate the reaction quotient Qp and state whether the reaction proceeds to the right or to the left as equilibrium is approached
Chemistry
1 answer:
Ganezh [65]3 years ago
7 0

Answer:

To the right

Explanation:

Step 1: Given data

  • Partial pressure of PCl₅ (pPCl₅) = 0.548 atm
  • Partial pressure of PCl₃ (pCl₃) = 0.780 atm
  • Partial pressure of Cl₂ (pCl₂) = 0.780 atm

Step 2: Write the balanced equation

PCl₅(g) ⇄ PCl₃(g) + Cl₂(g)

Step 3: Calculate the pressure reaction quotient

Q_p = \frac{pPCl_3 \times pCl_2 }{pPCl_5} = \frac{0.780 \times 0.780 }{0.548} =1.11

Step 4: Determine whether the reaction proceeds to the right or to the left as equilibrium is approached

Since <em>Qp < Kp</em>, the reaction will proceed to the right to attain the equilibrium.

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Answer:

Answers are in the explanation.

Explanation:

<em>Given concentrations are:</em>

  • <em>SO₂ = 0.20M O₂ = 0.60M SO₃ = 0.60M</em>
  • <em>SO₂ = 0.14M O₂ = 0.10M SO₃ = 0.40M </em>
  • <em>And SO₂ = 0.90M O₂ = 0.50M SO₃ = 0.10M</em>

<em />

In the reaction:

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<em />

Also, you can define Q (Reaction quotient) as:

Q = [SO₃]² / [O₂] [SO₂]²

<em>Where concentrations of each species are ACTUAL concentrations.</em>

<em />

If Q > Kc, the reaction will shift to the left until Q = Kc;

If Q < Kc, the reaction will shift to the right until Q = Kc

If Q = Kc, there is no net reaction because reaction would be en equilibrium.

Replacing with given concentrations:

  • Q = [0.60M]² / [0.60M] [0.20M]² = 15; Q = Kc → No net reaction
  • Q = [0.40M]² / [0.10M] [0.14M]² = 82; Q > Kc, → Reaction will shift to the left
  • Q = [0.10M]² / [0.50M] [0.90M]² = 0.015; Q < Kc → Reaction will shift to the right

<em />

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