The rate constant of a reaction is `1.5 xx 10^(7)s^(-1)` at `50^(@)C` and `4.5 xx 10^(7) s^(-1)` at `100^(@)C`. Evaluate the Arrhenius parameters `A` and `E_(a)`.

The rate constant of a reaction 1.5xx10^(7)s^(-1) " at " 50^(@)C and 4.5xx10^(7)s^(-1) at 100^(@)C Evaluate the Arrhenius parameters A and E_(a)

the rate constant of a reaction is 1.5xx10^(7) s^(-1) at 50^(@)C and 4.5 xx10 ^(7) s^(-1) at 100 ^(@)C. Evaluate the Arrhenius paraments A and E^(a) . (ii) for the reaction N_(2)O_(5)(g) to 2NO_(2)(g) + 1/2 O_(2)(g) calculate the mole fractions N_(2)O_(5)(g) decomposed at a constant valume and temperature , if the initial pressses os 600 mm Hg and the pressure at any time is 960 mm Hg Assume ideal gas behaviour.

The rate constant of a reaction is 1.5xx10^(-4)s^(-1)" at "27^(@)C and 3xx10^(-4)s^(-1)" at "127^(@)C . The Ea is

The rate constant of a reaction is 1.5xx10^(-4)s^(-1)" at "27&(@)C and 3xx10^(-4)s^(-1)" at "127^(@)C . The Ea is

The rate constant for a reaction is 1.5 xx 10^(-7) at 50^(@) C and 4.5 xx 10^(7)s^(-1) at 100^(@) C . What is the value of activation energy?

The rate constant for a reaction is 1.5 xx 10^(-7) at 50^(@) C and 4.5 xx 10^(7)s^(-1) at 100^(@) C . What is the value of activation energy?

The rate constant of a reaction is 1.5 xx 10^(7)s^(-1) at 50^(@) C and 4.5 xx 10^(7)s^(-1) at 100^(@) C. Calculate the value of activation energy for the reaction (R=8.314 J K^(-1)mol^(-1))