The oxidation of ammonia takes place as,
`4NH_(2)(g)rarr3O_(2)(g)rarr2N_(2)(g)+6H_(2)O(g)` If the rate of formation of `N_(2) "is" 0.7 M//s`, detemine the rate at which `NH_(3)` is consumed.

The oxidation of ammonia produces nitrogen and water according to the equation : 4NH_(3)(g)+3O_(2)(g)rarr2N_(2)(g)+6H_(2)O(g) If the rate of formation of N_(2) at a certain temperature is 3.0"mol.L^(-1).s^(-1) , what is the rate of disappearance of O_(2) ?

For the reaction : 2 NH_(3)(g) rarr N_(2)(g) + 3 H_(2)(g)

For the reaction , 2C_(2)H_(6)(g)+7O_(2)(g)rarr4CO_(2)(g)+6H_(2)O(l) , the rate of disappearnce of C_(2)H_(6)(g) :

In the reaction 4NH_(3)+3O_(2(g)) to 2N_(2(g))+6H_(2)O_((g))

The commercial poduction of ammonia is represented by the equation, N_(2)(g)+3H_(2)(g)rarr2NH_(3)(g) . If the rate of disappearance of H_(2)(g) is 1.2xx10^(-3) mol/min, what is the rate of appearance of NH_(3)(g) ?

For the reaction 2N_(2)O_(5)(g)rarr4NO_(2)(g)+O_(2)(g) the rate of formation of NO_(2)(g)" is "2.8xx10^(3)(M).s^(-1) . Calculate the rate of disappearance of N_(2)O_(5)(g) .

The differential rate law for the reaction, 4NH_3(g)+5O_2(g)rarr4NO(g)+6H_2O(g)

The differential rate law for the reaction, 4NH_3(g)+5O_2(g)rarr4NO(g)+6H_2O(g)

The standard enthyalpy of N_(2(g))+3H_(2(g)rarr2NH_(3(g)) is