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19 December, 02:58

Which situation would cause the following equilibrium reaction to decrease the formation of products 2SO2 (g) + O2 (g) forward backward arrow 2SO43 (g) + energy

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  1. 19 December, 03:37
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    The reaction is as Follow,

    2 SO₂ + O₂ ⇄ 2 SO₃ ΔH = - 94.58 kJ mol⁻¹

    Changing Concentration:

    According to Le Chatelier's principle, the removal of SO₂ and O₂ (or decrease in their concentration) at equilibrium will result in decrease in the formation of SO₃.

    Changing Pressure:

    As the reaction proceeds by the decrease in volume, so by decreasing the pressure will shift the equilibrium in backward direction decreasing the concentration of product.

    Changing Pressure:

    Since the forward reaction is exothermic, the equilibrium will be shifted in backward direction by increasing the temperature.
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