The oxidation of ammonia produces nitrogen and water via the following reaction: 4nh3(g) + 3o2(g) → 2n2(g) + 6h2o(l) suppose the rate of formation of h2o(l) is 3.0 mol/(l ∙ s). which of the following statements is true? a. the rate of consumption of nh3 is 0.50 mol/(l ∙ s). b. the rate of consumption of nh3 is 2.0 mol/(l ∙ s). c. the rate of formation of n2 is 2.0 mol/(l ∙ s). d. the rate of formation of n2 is 1.3 mol/(l ∙ s). e. the rate of consumption of o2 is 2.0 mol/(l ∙ s).

The rate of consumption of is 2.0 mol/L.s

Explanation:

Applying law of mass action to this reaction-

where represents rate of consumption of , represents rate of consumption of , represents rate of formation of and represents rate of formation of .

Here rate of formation of is 3.0 mol/(L.s)

From the above equation we can write-

Here

So,

Hence,  

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.