Consider the reaction at equilibrium 2KCl(s) + 3O2(g) = 2KClO3(s), Which way wou

ID: 871945 • Letter: C

Question

Consider the reaction at equilibrium 2KCl(s) + 3O2(g) = 2KClO3(s),

Which way would the reaction shift (left, right, stay the same) of the following changes:

O2 added to the reaction mixture

KCl added to the reaction mixture

KClO3 removed from the reaction mixture

Volume of the reaction vessel increased

Consider the endothermic gas phase reaction at equilibrium, C2H4Cl2 = C2H4 + Cl2

Which way would the reaction shift (left, right, stay the same) of the following changes:

Adding more Cl2 to the reaction mixture

Raising the temperature

Adding a catalyst

Adding argon gas to the reaction

Increasing the volume of the reaction vessel

For each of these, can you please provide a quick explaination? I have trouble understanding le chatelier's principles

Consider the reaction at equilibrium 2KCl(s) + 3O2(g) = 2KClO3(s)

O2 added to the reaction mixture - shifts right

KCl added to the reaction mixture - no effect (its a solid cant participate in the equilibrim process)

KClO3 removed from the reaction mixture - no effect

Volume of the reaction vessel increased- reaction shifts to left.

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Consider the endothermic gas phase reaction at equilibrium, C2H4Cl2 = C2H4 + Cl2 , DH = +ve

Adding more Cl2 to the reaction mixture

Raising the temperature - reaction shifts to left

Adding a catalyst - stay the same but rate of forward reaction increases

Adding argon gas to the reaction- no effect at constant volume

Increasing the volume of the reaction vessel- reaction shifts to right.