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NO(2) dimerises to form N(2)O(4). Why?...

`NO_(2)` dimerises to form `N_(2)O_(4)`. Why?

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Why NO_2 dimerise to N_2O_4 ?

Which is not correct for N_2O ?

The value of rate constant for the decomposition of nitrogen pentoxide (N_(2) O_(s) to N_(2) O_(4) + (1)/(2) O_(2) ) is 3.46 xx 10^(-5) at 25^(@) C and 4.87 xx 10^(-3) at 65^(@) C . Calculate the energy of activation for the reaction. ( R = 8.314JK^-1mol^-1 )

The possible mechanism for the reaction 2NO(g) + O_(2)(g) to 2NO_(2) is (i) NO + O_(2) to NO_(3) (fast) (ii) NO_(3) + NO to K_(2) NO_(2) + NO_(2)(g) (slow) write the rate law and order for the reaction.

For the decomposition of N_(2) O_(5) given as, N_(2) O_(5) (g) to N_(2) O_(4) (g) + 1//2O_(2) (g) If the rate law =K [N_(2) O_(5) ] and K=1.68 xx 10^(-2)" s"^(-1) , starting with 2.5 moles, of N_(2) O_(5)(g) in a 5.0"L" container at 298K, how many moles of N_(2) O_(5) would remain after 1.0 minutes?

The experimental data for the decomposition of N_(2) O_(5) , [2N_(2) O_(5) to 4NO_(2) + O_(2)] in gas phase of 318 K are given below: Find the half-life period for the reaction.