A) \[\Delta G<0;\text{ }\Delta S>0;\text{ }\Delta H<0\]
B) \[\Delta G<0;\text{ }\Delta S<0;\text{ }\Delta H<0\]
C) \[\Delta G>0;\text{ }\Delta S>0;\text{ }\Delta H<0\]
D) \[\Delta G<0;\text{ }\Delta S<0;\text{ }\Delta H>0\]
E) \[\Delta G>0;\text{ }\Delta S>0;\text{ }\Delta H>0\]
Correct Answer: B
Solution :
Adsorption is an exothermic process and hence,\[\Delta H\]is negative for adsorption. On the other hand the molecules of the adsorbate are held on ±e surface of the adsorbent and hence, they have lesser tendency to move about freely. In other words entropy decreases i.e.,\[\Delta S\]is negative. According to Gibbs-Helmholtz equation, \[\Delta G=\Delta H-T.\Delta S\] Thus for the process of adsorption to occur \[\Delta G\]must be negative. Hence, for adsorption \[\Delta G<0;\Delta S<0;\Delta H<0\]
You need to login to perform this action.
You will be redirected in
3 sec
