Effect of temperature of equilibrium constant is given by `logK_(2)-logK_(1)=(-DeltaH)/(2.303R)[(1)/(T_(2))-(1)/(T_(1))](" where "T_(2)gtT_(1))`. Then for a endothermic reaction the false statement is

The effect of temperature on equilibrium constant is expressed as (T_(2)gtT_(1)) log K_(2)//K_(1)=(-DeltaH)/(2.303)[(1)/(T_(2))-(1)/(T_(1))] . For endothermic, false statement is

The effect of temperature on equilibrium constant is expressed as (T_(2)gtT_(1)) log K_(2)//K_(1)=(-DeltaH)/(2.303)[(1)/(T_(2))-(1)/(T_(1))] . For endothermic, false statement is

Assertion : The equilibrium constant of an exothermic reaction decreases as temperature increases. Reason : log(K_(2)/K_(1))=(DeltaH)/(2.303R)(1/T_(1)-1/T_(2)) where T_(2) gt T_(1) . Since for an exothermic reaction DeltaH is -ve, it follows that K_(2)/K_(1) lt 1 or K_(2) lt K_(1) .

STATEMENT-1: The equilibrium constant of the exothermic reaction at high temperature decreases. STATEMENT-2: Since In (K_(2))/(K_(1))=(DeltaH^(@))/(R)[(1)/(T_(1))-(1)/(T_(2))] and for exothermic reaction , DeltaH^(@)= -ve and thereby, (K_(2))/(K_(1))lt1

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)] Select the correct statement :

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)] Select the correct statement :