The activation energy for the reactio `2HI_((g))to H_(2(g))+I_(2(g))at 581` K is `209. 5kJ//mol.` Calculte the fraction of molecules having energy equal to or grater than activation energy. `[R=8.31 JK^(-1)mol ^(-1)]`

The activiation energy for the reaction 2HI(g) to H_(2) + I_(2)(g) is 209.5 KJ mol^(-1) at 581 K.Calculate the farction of molecules of reactants having energy equal to or greater than activation energy ?

If the activation energy for the forward reaction is 150kJ mol^(-1) and that of the reverse reaction is 260kJ mol^(-1) . What is the enthalpy change for the reaction

The first order rate constant for the decomposition of ethyl iodide by the reaction. C_(2)H_(2)I (g)to C_(2)H_(4) (g)+ HI (g)at 600K is 1.60 xx10^(-5)s^(-1). It is energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700 K.

The kinetic energy in J of 1 mole of N_2 at 27^@ C is (R= 8.314 mol^(-1) k^(-1))

Kinetic energy in Kj of 280 g of N_(2) at 27^(@)C is approximately (R = 8. 314 J mol ^(-1) K ^(-1))

N_(2(g))+3H_(2(g))hArr2NH_(3)(g)+22k.cal . The activation energy for the forward reaction is 50 k. cal What is the activation energy for the backward reaction ?

The energies of activation for forward and reverse reactions for A_(2)+B_(2)to2AB are 280kJ"mol"^(-1) and 400kJ"mol"^(-1) respectively. The presence of catalyst lowers the activation energy of both forward as well as reverse reactions by 100KJ"mol"^(-1) . The enthalpy change of the reaction A_(2)+B_(20to2AB in the presence of catalyst will be (in KJ "mol"^(-1) )

The molar entropies of HI_((g)), H_((g)) and I_((g)) at 298K are 206.5, 114.6, and 180.7 J mol^(-1)K^(-1) respectively. Using the DeltaG^(@) given below, calculate the bond energy of HI. HI_((g)) rarr H_((g)) + I_((g)), DeltaG^(@) = 271.8kJ (Give your answer after divide with 49.7)

At T(K), the ratio of kinetic energies of 4g of H_(2) (g) and 8g of O_(2) (g) is