Please explain Consider this gas phase system at equilibrium: PCls(g) PCI_3(g) +

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Please explain

Consider this gas phase system at equilibrium: PCls(g) PCI_3(g) + CI_2(g) Delta H degree _rxn = +87.8 kJ/mol. Which of these statements is false? A) Increasing the system volume shifts the equilibrium to the right. B) Increasing the temperature causes the equilibrium constant to increase. C) A catalyst speeds up the approach to equilibrium and shifts the position of equilibrium to the right. D) Decreasing the total pressure of the system shifts the equilibrium to the right E) None of these is false At 700 K, the reaction 2SO_2(g) + O_2(g) 2SO_3(g) has the equilibrium constant K_c = 4.3 times 10^6 Suppose the following concentrations are present in a mixture: [SO_2] = 0.10 M; [SO_3] = 10. M; [O_2] = 0.10 M. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written), left to right or right to left, will the reaction proceed to reach equilibrium? A) Yes, the mixture is at equilibrium. B) No, left to right D) There is not enough information to be able to predict the direction. E) None of the above

Explanation / Answer

9) The reaction is endothermic in nature thus, increasing the temperature shifts the equilibrium to right and hence equilibrium constant value increases. Moreover, with the decrease in pressure, volume increases and equlibrium shifts in a direction where there is more number of moles i.e. the current equilibrium shifts to right. All these generalisations are in accordance with Lechateliers principle.

However, catalyst enhances the rate of reaction and incase of an equlibrium it enhances the rate of both forward and backward reaction. as a result of which it does not have any effect on equilibrium and no shifting of equilibrium takes place.

statement C is false

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