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accoording to the arrhnius equation the rate constant of any reaction increases with increase of temp .............yet the rate const of an exothermic rxn decreases with increase of temp....why is that??



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i want an AIEEE guide or a book which has collection of previous years' questions of AIEEE




how do i calculate the n factor of Cl2 in the following disproportionation reactionNaOH + Cl2 >NaCl + NaClO3remember that in the above reaction Cl2 has been reduced to NaCl and oxidised to NaClO3....



well i can understand its phyical significance as energy of molecules of water increase U also should increase but i cant explain it in terms of thermodynamical parameters as deltaU should be 0 if temp remains const.another thing is that right above this question they have derived an expression for deltaH=deltaU+deltaN(g)*R*T....why is it that in the derivation they have assumed...... pV(A)=n(A)*R*T.............(1) pV(B)=n(B)*R*T..............(2) SO BASICALLY THEY HAVE ASSUMED THAT TEMP AT STATE A AND STATE B IS SAME AND EQUAL TO T.....BUT IF THTS TRUE THEN YET AGAIN "DELTA U" OF THE REACTION BECOMES ZERO PS:everything given in brackets is the subscript



hey guys!!my doubt is based on thermodynamics.well on pg161 of NCERT we have problem 6.5 in which in the first part they've asked us to calculate deltaU.now if the phase transformation is at const temp why should there be a change in U??well i can understand its phyical significance as energy of molecules of water increase U also should increase but i cant explain it in terms of thermodynamical parame


