PCls(g) > PCI, (g) + Cl2(g) For the reaction above, = +22.1 kilocalories per mol

Question

PCls(g) > PCI, (g) + Cl2(g) For the reaction above, = +22.1 kilocalories per mole at 25 degree C. Does the tendency of reactions to proceed to state of minimum energy favor the formation of the products of this reaction? Explain. Does the tendency of reactions to proceed to a state of maximum entropy favor the formation of the products of this reaction? Explain. State whether an increase in temperature drives this reaction to the right, to the left, or has no effect. Explain. State whether a decrease in the volume of the system at constant temperature drives this reaction to the right, to the left, or has no effect. Explain.

Explanation / Answer

We Know that :          The givenreaction is:           PCl5 (g) --------> PCl3(g) +   Cl2 (g)          The abovereaction tends to form at the condition of the minimum energy whichis been observed with respect to           thenegative value of the G. which indicates the formation of theabove products.           Theabove reaction tends to form with rtespect to the maximum entropyas the number of gaseous moles increases             withrespect to the product formed so the entropy increases.           As the reaction is endothermic so the increase in temperaturedrives the reaction in the forward direction.           For the above reaction decrease in volume at constanttemperature favours forward reaction where their is increase             in volume with respect to number of moles.              

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