The decomposition of `N_(2)O` into `N_(2)` and O in the presence of gaseous argon follows second kinetics with
`k=(5.0xx10^(11)` L `"mol"^(-1) s^(-1))e^(-29000 K//T)`
The energy of activation is

The decomposition of N_(2)O into N_(2) and O in the presence of gaseous argon follows second order kinetics with k=(5.0xx10^(11) L " mol"^(-1)s^(-1))e^(-29000 K//T) The activation energy for the reaction E_(a) is

The decomposition of N_(2)O into N_(2) & O_(2) in presence of gaseous argon follow second order kinetics with k = (5.0 xx 10^(11) L "mol"^(-1) s^(-1)) e^(-(41570)/(T))" " (K stands for Kelvin units). The energy of activation of the reaction is

The decomposition of N_(2)O into N_(2) and O_(2) in presence of gaseous argon follows second order kinetics with rate constant, K=5.0 xx10^(11) e^(-30000K//T)mol^(-1)s^(-1) . The enrgy of activation are respectively (R=2 cal K^(-1) mol^(-1))

The decomposition of N_(2)O in N_(2) and O_(2) in presence of gaseous argon follows II order kinetics having K=5xx10^(11) e^(-29000//T) . Find out energy of activation and rate constant at 27^(@)C . Also evalute Arrhenius parameter.

The decomposition of N_(2)O into N_(2) and O_(2) in presence of gaseous argon follows second order kinetics with rate constant, K=2.0 xx10^(11) e^(-30000K//T)mol^(-1)s^(-1) . The pre - exponential factor and the enrgy of activation are respectively (R=2 cal K^(-1) mol^(-1))

The decomposition of N_2O into N_2 and O_2 follows second order kinetics with k = (5.0 xx 10^(11) L "mol"^(-1) s^(-1)) e^(-(41570)/(T))" , it suggests that

The decompostion of N_(2)O into N_(2) and O_(2) in presence of Argon follows first order kinetics k=5.0xx10^(11)e^(-2000//T(K)) . The activation energy is