When the number of molecules in a container decreases in a chemical reaction the reactants probability of collision decreases thus it will slow the reaction, however if the volume of the container decreases the reaction is favored, for example: if the following reaction is at equilibrium: 3O2(g) ←→ 2O3(g) and it is transfer to a small vessel, the products will be favored. The opposite is true, if following reaction 2CO2(g) ←→ 2CO(g) + O2(g) is transferred to a smaller container the reaction will be favored toward the reactants. Would decreasing the volume of the container for each of the following reactions cause the equilibrium to shift in the direction of products, reactants, or no change? a. P4(g) +5O2(g) ←→ P4O10(s) b. 2SO2(g) + 2H2O(g) ←→ 2H2S(g) + 3O2(g)
When the number of molecules in a container decreases in a
Would decreasing the volume of the container for each of the following reactions cause the equilibrium to shift in the direction of products, reactants, or no change?
a. P4(g) +5O2(g) ←→ P4O10(s)
b. 2SO2(g) + 2H2O(g) ←→ 2H2S(g) + 3O2(g)
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