2SO2 2 (g) ( g ) + O2 2 (g) ( g ) ↔ 2SO3 3 (g) ( g ) ΔH = -395.7kJmol−1 − 1 In the equation, an increase in temperature will shift the equilibrium position ...

Question 1 Report

2SO $_{2}$ $_{(g)}$ + O $_{2}$ $_{(g)}$ ↔ 2SO $_{3}$ $_{(g)}$ ΔH = -395.7kJmol $^{- 1}$

In the equation, an increase in temperature will shift the equilibrium position to the

left and equilibrium constant decreases

left and equilibrium constant increases

right and equilibrium constant increases

right and equilibrium constant decreases

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