The equilibrium constant K₁, K2 and K3 for the reactions below areS(s) + O₂(g) → SO₂(g), K₁ = 4.2 × 10522S (s) +30₂(g)2SO3(g),K₂ = x2SO2(g) + O2(g)2SO3(g),The value of K₂ is9.8 × 10282.6 × 1075□ 6.7 × 10¹21.34 × 10329.8 x 10128K3= 5.6 x 1023

We can get equation 2 by adding equation 1 and 3 equation. We know that if we multiply any constant…

The equilibrium constant K₁, K2 and K3 for the reactions below are S(s) + O₂(g) → SO₂(g), K₁ = 4.2 × 1052 2S (s) +302(g)2SO3(g), 2SO2(g) + O2(g) =2SO3(g), The value of K₂ is ☐ O 9.8 × 1028 2.6 × 1075 6.7 × 10¹2 1.34 × 1032 9.8 x 10128 K₂ = x K3 = 5.6 × 102³

The equilibrium constant K₁, K2 and K3 for the reactions below are S(s) + O₂(g) → SO₂(g), K₁ = 4.2 × 1052 2S (s) +302(g)2SO3(g), 2SO2(g) + O2(g) =2SO3(g), The value of K₂ is ☐ O 9.8 × 1028 2.6 × 1075 6.7 × 10¹2 1.34 × 1032 9.8 x 10128 K₂ = x K3 = 5.6 × 102³

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 56QRT

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Question

The equilibrium constant K₁, K2 and K3 for the reactions below are
S(s) + O₂(g) → SO₂(g), K₁ = 4.2 × 1052
2S (s) +30₂(g)2SO3(g),
K₂ = x
2SO2(g) + O2(g)2SO3(g),
The value of K₂ is
9.8 × 1028
2.6 × 1075
□ 6.7 × 10¹2
1.34 × 1032
9.8 x 10128
K3= 5.6 x 1023

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