Consider the following equilibrium: 2 SO2 (g) + O2(g) = 2 SO3 (g), delta H = -19

Question

Consider the following equilibrium: 2 SO2 (g) + O2(g) = 2 SO3 (g), delta H = -198.2 kJ/mol Choose the TRUE statements from among the following: i) The equilibrium constant expression is K = [SO3]^2/[SO2]^2[O2]. ii) Reducing the volume of the container would shift the equilibrium to the right. iii) Adding more O2 would shift the equilibrium to the right. iv) Raising the temperature would shift the equilibrium to the right. v) Changing the temperature would affect the magnitude of the equilibrium constant. i and ii ii and iv i, iv, and v i, ii, iii, and v

Explanation / Answer

Option 4. i, ii, iii, v (True)

(iv) false.

Since, it is exothermic reaction, The rise in temperature would not shift equilibrium towards right.

-198.2 KJ /mol heat is released during the forward reaction.

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