In the hober's process of ammonia manufacture,
`N_(2)(g)+3H_(2)(g) rarr2NH_(3)(g)`
the rate of appearance of `NH_(3)` is :
`(d[NH_(3)])/(dt)=2xx10^(-4)"mol" L^(-1)"sec"^(-1)`
The rates of the reaction expressed in terms of `N_(2) and H_(2)` will be :

In the manufacture of NH_(3) by Haber process N_(2)(g) + 3H_(2)(g) to 2NH_(3)(g) the rate of the reaction was measured as - (d[N_(2)])/(dt) = 2 xx 10^(-4) "mol" L^(-1)s^(-1) . The rate of the reaction expressed in terms of H_2 is:

In a reaction N_(2(g))+3H_(2(g))to2NH_(3(g)) rate of appearance of NH_(3) is 2.5xx10^(-4)molL^(-1)sec^(-1) then rate of reaction and rate of disappearance of H_(2) respectively is :-

In a reaction N_(2(g))+3H_(2(g))to2NH_(3(g)) rate of appearance of NH_(3) is 2.5xx10^(-4)molL^(-1)sec^(-1) then rate of reaction and rate of disappearance of H_(2) respectively is :-

In a catalytic experiment involving Haber's process, N_(2)(g)+3" H"_(2)(g)to2" NH"_(3)(g) , the rate of reaction was measured as : Rate =(d[NH_(3)])/(dt)=2.0xx10^(-4)"M s"^(-1) . If there were no side reactions, what was the rate of reaction expressed in terms of N_(2) ?

The rate of formation of ammonia by the reaction: N_2+3H_2rarr2NH_3 expressed as (d[NH_3]/(dt))=2.5xx10^(-4)mol L^(-1) s^(-1) The rate of consumption expressed in terms of H_ 2 as (-d[H_2]/(dt)) will be