Chemical Kineti...

N₂ (g) + 2H₂ (g) ⇌ 2NH₃ (g) + 22 kcal
The activation energy for the forward reaction is 50 kcal. What is the activation energy for the backward reaction?

A given sample of milk turns sour at room temperature (27°C) in 5 h. In a refrigerator at -3° C, it can be stored 10 times longer. The energy of activation for the souring of milk is

The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol^{- 1} . The ratio of rate constant to the Arrhenius factor is

The activation energy of exothermic reaction A → B 80 kJ mol^-1 . The heat of reaction is 200 kJ mol^-1. The activation energy for the reaction B → A (in kJ mol^-1 ) will be

For a first order reaction A → P, the temperature (T) dependent rate constant (k) was found to follow the equation log k = - (2000) / T + 6.0
The pre-exponential factor A and the activation energy E_a, respectively, are

The energies of activation for forward and reverse reactions for A₂ + B₂ ⇌ 2AB are 180 kJ mol^-1 and 200 kJ mol^-1 respectively. The presence of a catalyst lowers the activation energy of both (forward and reverse) reactions by 100 kJ mol^-1. The enthalpy change of the reaction (A₂ + B₂ → 2AB)in the presence of catalyst will be (in kJ mol^-1)

Rate of a reaction can be expressed by Arrhenius equation as k = Ae^-E/RT In this equation, E represents

The rate constant of a first order reaction at 27°C is 10^-3 min ^-1. The temperature coefficient of this reaction is 2. What is the rate constant (in min ^-1) at 17°C for this reaction ?

Arrhenius equation is

Consider an endothermic reaction X →Y with the activation energies E_b and E_f for the backward and forward reactions respectively. In general