If `K_(1)` and `K_(2)` are equilibrium constants at `T_(1)` and `T_(2)` temperatures (`T_(1)`>`T_(2)`) ,then which of the following are correct?
(A) When `Delta` H=+ve,`K_(2)`>`K_(1)`
(B) When `Delta` H=0 `K_(1)`=`K_(2)`
(C) When `Delta` H=-ve `K_(2)`<`K_(1)`
(D) When `Delta` H=+ve `K_(2)`<`K_(1)`

If K_(1)= Rate constant at temperature T_(1) and k_(2) rate constant at temperature T_(2) for a first order reaction, then which of the following relation is correct ?

For an exothermic reaction, equilibrium constant at T_1 and T_2 are respectively K_1 and K_2 If K_1 lt K_2 then : -

chi_(1) and chi_(2) are susceptinilities of diamagnetic substance at temperatures T_(1)K and T_(2)K respectively. Then

If K_1 is the equilibrium constant at temperature T_1 and K_2 is the equilibrium constant at temperature T_2 and If T_2 gt T_1 and reaction is endothermic then

Activation energy (E_(a)) and rate constants ( k_(1) and k_(2) ) of a chemical reaction at two different temperatures ( T_(1) and T_(2) ) are related by

If K_(1) represents the equilibrium constant for reaction: H_(2)+I_(2)hArr2HI & K_(2)" for "(1)/(2)H_(2)+(1)/(2)I_(2)hArr HI the relation between K_(1)& K_(2) would be

Variation of equilibrium constan K with temperature is given by van't Hoff equation InK=(Delta_(r)S^(@))/R-(Delta_(r)H^(@))/(RT) for this equation, (Delta_(r)H^(@)) can be evaluated if equilibrium constans K_(1) and K_(2) at two temperature T_(1) and T_(2) are known. log(K_(2)/K_(1))=(Delta_(r)H^(@))/(2.303R)[1/T_(1)-1/T_(2)] For an isomerization X(g)hArrY(g) the temperature dependency of equilibrium cohnstant is given by : lnK=2-(1000)/T The value of Delta_(r)S^(@) at 300 K is :