The decomposition of dinitrogen pentoxide `(N_(2)O_(5))` follows first order rate law. Calculate the rate constant from the given data:
`t=800sec[N_(2)O_(5)]=1.45 "mol"L^(-1)=[A_()]`
`t=1600 sec [N_(2)O_(5)]=0.88"mol"L^(-1)=[A_(2)]`

The decomposition of dinitrogen pentoxide (N_(2)O_(5)) follows first order rate law. Calculate the rate constant from the given data: t=800sec[N_(2)O_(5)]=1.45 "mol"L^(-1)=[A_()] t=600 sec [N_(2)O_(5)]=0.88"mol"L^(-1)=[A_(2)]

If the decomposition of nitrogen oxide as 2N_2O_5 to 4NO_2 + O_2 follows a first order kinetics . Calculate the rate constant for a 0.05M solution if the instantaneous rate is 1.5 xx10^(−6) mol/l/s ?

The decomposition of N_(2)O_(5) in a carbon tetrachloride solutioin has been investigated. N_(2)O_(5)("solution") to 2NO_(3) (solution) + 1//2O_(2)(g) ltrbgt The reaction has been found to be of the first order in N_(2)O_(5) with a first order rate-constant = 6.2 xx 10^(-4)s^(-1) . Calculate the rate of the reaction when (a) [N_(2)O_(5)] = 1.25 mol L^(-1) and b) [N_(2)O_(5)] = 0.25 mol L^(-1) . c) What concentration of N_(2)O_(5) would give a rate of 2.4 xx 10^(-3) mol L^(-1)s^(-1) ?

The decomposition of nitrogen pentoxide is given as 2N_(2)O_(5) to 4NO_(2) + O_(2) . The rates of reaction are ([N_(2)O_(5)])/(Delta t ) =k_(1)[N_(2)O_(5)],(Delta[NO_(2)])/(Deltat) = k_(2) [N_(2)O_(5)] and (Delta [O_(2)])/(Delta t) = k_(3) [N_(2)O_(5)] Relate the rate constants k_(1) , k_(2) and k_(3) .

The decomposition of N_(2)O_(5) takes place according to I order as: 2N_(2)O_(5) rarr 4NO_(2)+O_(2) Calculate: (a) The rate constant, if instantaneous rate is 1.4 xx 10^(-6) mol litre^(-1) sec^(-1) when concentration of N_(2)O_(5) is 0.04M . (b) The rate of reaction when concentration of N_(2)O_(5) is 1.20 M . (c ) The concentration of N_(2)O_(5) when the rate of reaction will be 2.45 xx 10^(-5) mol litre^(-1) sec^(-1)