2N_(2)O_(5)rightleftharpoons DN_(2)O_(4)+O_(2)N

N_(2)O_(5) decomposes to N_(2)O_(4) and O_(2) as N_(2)O_(5) rarr N_(2)O_(4) + (1)/(2)O_(2) The pressure p_(t) at any stage is related to p_(0) and 'x', the fraction of dissociation, as :

For the first-order decomposition reaction of N_(2)O_(5) written as: 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) , rate =k[N_(2)O_(5)] N_(2)O_(5)(g) to 2NO_(2)(g) + 1/2O_(2)(g) , rate =k'[N_(2)O_(5)] which of the following facts is true?

(A) N_(2)O_(5) is more acidic than N_(2)O_(4) (R ) N_(2)O_(4) is a mixed anhydride where as N_(2)O_(5) is not

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 reaction 2N_(2)O_(5)hArr 2N_(2)O_(4)+O_(2) is

2N_(2)O_(5) rarr 4NO_(2) + O_(2) If (-d[N_(2)O_(5)])/(dt) = k_(1)[N_(2)O_(5)] (d[NO_(2)])/(dt) = k_(2)[N_(2)O_(5)] (d[O_(2)])/(dt) = k_(3)[N_(2)O_(5)] What is the relation between k_(1), k_(2) , and k_(3) ?

If alpha is the degree of dissociation of N_(2)O_(4) in the reaction : N_(2)O_(4)hArr 2NO_(2) then at equilibrium, the total number of moles of N_(2)O_(4) and NO_(2) present is :