In the reaction : `N_(2)+3H_(2)rarr2HN_(3)` the rate of formation of `NH_(3) " is " 9.6xx10^(-3)"mol.L"^(-1).s^(-1). ` Calculate the rates of disappearance of `N_(2) and H_(2)` .

Explanation

Rate of the given reaction
`=-(Delta[N_(2)])/(Deltat)=-(1)/(3)(Delta[H_(2)])/(Deltat)=(1)/(2)(Delta[NH_(3)])/(Deltat)" "...[1]`
Given : `(Delta[NH_(3)])/(Deltat)=9.6xx10^(-3)"mol. L"^(-1).s^(-1)` From equation [1],
we get the rate of disappearance of `N_(2)` ,
`-((Delta[N_(2)])/(Deltat))=(1)/(2)xx " rate of formation of "NH_(3),((Delta[NH_(3)])/(Deltat))`
`=(1)/(2)xx9.6xx10^(-3)=4.8xx10^(-3)"mol L"^(-1).s^(-1)`
and rate of disappearance of `H_(2)` ,
`(-(Delta[H_(2)])/(Deltat))=(3)/(2)xx` rate of formation of `NH_(3),((Delta[NH_(3)])/(Deltat))`
`=(3)/(2)xx9.6xx10^(-3)=1.44xx10^(-2)"mol L"^(-1).s^(-1)`