[" For n butane "rightleftharpoons" |sobutane "],[log_(e)K=4.0-(2000)/(T)],[" What is "Delta S^(@)" at "400k(" in Cals) ")]

For an isomerisation reaction, A hArr B , the temperature dependence of equilibrium constant is given by Log_0K=4.0 -(2000)/T Find the value of DeltaS^0 at 300 k in cal.

For an isomerisation reaction, A hArr B , the temperature dependence of equilibrium constant is given by Log_0K=4.0 -(2000)/T Find the value of DeltaS^0 at 300 k in cal.

The temperature dependence of equilibrium constant of a reaction is given by ln K_(eq) = 4.8 -(2059)/(T) . Find Delta_(r)G^(Theta), Delta_(r)H^(Theta), Delta_(r)S^(Theta) at 298 K

A reaction has value of Delta H = -40 kcal mol^(-1) at 400 K. Below 400 K the reaction is spontaneous and above 400 K it is not. The value of DeltaG and Delta S at 400 K are respectively

Rate constant k varies with temperature by equation, log k (min+^(-1))=5-(2000)/(T(K)) We can conclud:

Rate constant k varies with temperature by equation, log k (min+^(-1))=5-(2000)/(T(K)) We can conclud:

For the reaction A(s) rarr A(g) , the variation of log K_(P)^(@) us (1)/(T) is given by: If S_(m)^(@), A(g) is 31.78 cal//K mole, then calculate S_(m)^(@) A(s) in cal/K mole.

One mole of an ideal gas (Y=1.5) compressed adiabatically from (8.0L,400K) to 4.0 L against constant external pressure of 8.314 bar. Calculate the value of 10 times of (Delta S)_(" total ") in (cal/ k) for the process (Given: ln2 =0.7,ln3 =1.1)

For a certain reaction log K (S^(-1))= 14- (1.25 xx 10^(4)K)/(T) Hence it can be said that The E_(a) for the reaction is