Use Le Chatelier’s Principle to predict whether the amount of PCl3 in a 1.00 –L

Question

Use Le Chatelier’s Principle to predict whether the amount of PCl3 in a 1.00 –L container increased, decreased or remains the same for the equilibrium PCl3(g) + Cl2(g) <=> PCl5(g) + heat when each of the following change is made.

When PCl5 is added PCl3 a)increases b)remains the same c)decreases

When Cl2 is added PCl a)increases b)remains the same c)decreases

When PCl5 is removed PCl3 a)increases b)remains the same c)decreases

When the temperature is decreased PCl3 a)increases b)remains the same c)decreases

When a catalyst is added PCl3 a)increases b)remains the same c)decreases

Explanation / Answer

According to Le Chatelier’s Principle if we increase the concentration of any species then the equilibrium shifted to opposite side of the species present.

If we increase the temperature then equilibrium shifted towards products for the andothermic reaction and equilibrium shifted towards reactants for the exothermic reactions.

In the given reaction heat is released so it is exothermic reaction.

1) when PCl5 is aaded amount of PCl3 a) increases. Becuase PCl3 is in opposite side of PCl5.

2) When Cl2 is added amount of PCl3 c)decreases. Becuase PCl3 is in same side of PCl5.

3) When PCl5 is removed amount PCl3 a)increases

4) When the temperature is decreased amount of PCl3 c)decreases. Because the rection is exothermic so decreasing temperature is products favored. Amount of PCl5 increases and amount of PCl3 decreases.

5)When a catalyst is added amount PCl3 b)remains the same. Because catalyst does not change the equilibrium concentrations of species.

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