The experimental data for decomposition of `N_2O_5` `2N_2O_5 rarr 4NO_2 + O_2` in gas phase at 318K are given below:

Calculate the half-life Period from k and compare it with (b) .

The experimental data for decomposition of N_2O_5 2N_2O_5 rarr 4NO_2 + O_2 in gas phase at 318K are given below: What is the rate law?

The rate constant for the decomposition of N_2O_6 , N_2O_6 rarr N_2O_4+1/2O_2 is 3.46 xx 10^(-5) at 25^@ C and 4.87 xx 10^(-3) at 65^@ C. Calculate the energy of activation of the reaction.

For the first order reaction 2N_2O_5 (g) rarr 4 NO_2(g)+ O_2(g) which is incorrect:-

Calculate the oxidation number of nitrogen (N) in N2O5

Complete the reaction : N_2O + NaNH_2 rarr

Calculate the oxidation number of Mn in K M n O 4

Calculate the oxidation number of Mn in K M n O 4

The decomposition of N_2O_5 according to the equation, 2N_2O_5(g) harr 4NO_2(g) + O_2(g) is a first order reaction. After 30 min from the start of the decomposition in a closed vessel, the total pressure developed is found to be 284.5 mm of Hg and on complete decomposition, the total pressure is 584.5 mm of Hg. Calculate the rate constant of the reaction.

Decomposition of NH_(4)NO_(2)(aq into N_(2)(g) and 2H_(2)O(l) is first order reaction.

The initial concentration of N_2O_5 in the following first order reaction N_2O_5(g) rarr 2 NO_2(g) + 1/2O_2 (g) was 1.24 x 10^(-2) mol L^(-1) Calculated the rate constant of the reaction at 318 K.