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a quantity of pcl5 was heated in a 10 litre vessel at 250°c pcl5(g)=pcl3(g)+cl2(g) at equilibrium the vessel contains 0.25 moles of pcl5 ,0.3 mole of pcl3 ,0.30 moles of cl2 a)compute the equilibrium constant for the formation of pcl5 at 250°c? b)what is deltaG° for the dissociarion of pcl5?[log0.036= -1.443] answer:- a)27.77 , 0.036 b) +14.45 kJ

a quantity of pcl5 was heated in a 10 litre vessel at 250°c
pcl5(g)=pcl3(g)+cl2(g)
at equilibrium the vessel contains 0.25 moles of pcl5 ,0.3 mole of pcl3 ,0.30 moles of cl2
a)compute the equilibrium constant for the formation of pcl5 at 250°c?
b)what is deltaG° for the dissociarion of pcl5?[log0.036= -1.443]
 
 
answer:-
a)27.77  , 0.036
b) +14.45 kJ

Grade:11

1 Answers

Avni Chauhan
askIITians Faculty 247 Points
5 years ago
572-1703_Capture answer.PNG

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