At a certain temperature, T K the endothermic reaction `ArarrB` proceeds completely to the end. Determine sign of `DeltaG (+or -)` for the reaction `BrarrA` at the temperature,T K.

In general it is observed that the rate of a chemical reaction doubles with every 10^(circ) rise in temperature. If this generalisation holds for a reaction in the temperature range 295 (~K) to 305 (~K) , what would be the value of activation energy for this reaction? (R)=8.314 (Jk)^(-1) (~mol)^(-1)

Assertion : The rate of reaction whether exothermic or endothermic, increases with temperature. Reason : The rate of reaction = K [reactant] and K increases with temperature.

The rate of a reaction quadruples when the temperature changes from 293 (~K) to 313 (~K) . Calculate the energy of activation of the reaction assuming that it does not change with temperature.

In Haber's process, ammonia is manufactured according to the following reaction N_(2(g)) + 3H_(2(g)) hArr 2NH_(3(g)) , Delta H^(@) = -2.4 kJ The pressure inside the chamber is maintained at 200 atm and temperature at 500^(@)C . Generally this reaction is carried out in presence of Fe catalyst. The preparation of ammonia by Haber's process is an exothermic reaction. If the preparation follows the following temperature pressure relationship for its % yield. Then for temperature T_(1), T_(2) and T_(3) , the correct option is :

For a 1st order reaction, time taken for half of the reaction to complete is t, whereas that for3/4 th of the reaction to complete is t_(2) . How are t_(1) and t_(2) , related to each other?

Assertion : E_(a) of the forward reaction is higher than that backward reaction in a reversible endothermic reaction. Reason: Increasing the temperature of the substance increase the fraction of molecules which collide with energies greater than E_(a) .