For a reaction suppose the activation energy Is zero. What is the value of rate constant at 300 K ? If K is `1.6xx10^8S^-1`at 280 K`(R=8.314 J K^-1mol^-1`.

The equilibrium constant for a reaction is 10. What will be the value of DeltaG^theta at 300 K

The temperature dependence of the rate of a chemical reaction can be accurately explained by Arrhenius equation. With the help of Arrhenius equation, calculate the rate constant for the first order reaction C_2H_5I(g)toC_2H_(4(g))+HI_((G))at700K .Energy of activation (Ea)for the reaction is 209kjmol_(-1) and rate constant at 600K is 1.60xx10^(-5)s^(-1) [Universal gas constant R= 8.314JK^(-1)mol^(-1)]

a) State Hess's Law of constant heat summation. b) The equilibrium constant for a reaction is 5. What will be tha value of DeltaG^0. Given that R = 8.314 JK^-1mol^-1 , T=300K. R = 8.314 JK^-1mol^-1 T = 300K

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)

The activation energy for a reaction which doubles the rate when the temperature is raised from 300 K to 310 K is

The rate constant, the activation energy and the Arrhenius parameters of a chemical reaction at 25^(@) C are 2.0 xx 10^(-5) s^(-1) , 100 kJ mol^(-1) and 6.0 xx 10^(14) s^(-1) , respectively. The value of rate constant at very high temperature approaches.

The rate constant of a chemical reaction at 280K is 1.6 xx 10^-6 s^-1 . The activation energy of this reaction is zero. The value of k for this reaction at 300K is