Question

For the reaction, \[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\], the rate of reaction is found to be 2 × 10⁻⁴ mol L⁻¹ s⁻¹. Calculate the rate of disappearance of Ni_(g) and that of H_2(g).

Answer 1

The given reaction is \[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\]

The rate of reaction = 2 × 10⁻⁴ mol L⁻¹ s⁻¹

Rate of disappearance of N₂:

From the reaction stoichiometry:

Rate of reaction = \[\ce{-\frac{d[N_2]}{dt}}\]

= \[\ce{-\frac{d[N_2]}{dt}}\]

= 2 × 10⁻⁴ mol L⁻¹ s⁻¹

Rate of disappearance of H₂:

From the stoichiometry:

\[\ce{1N2 + 3H2 -> 2NH3}\]

⇒ Rate of disappearance of H₂ = 3 × Rate of reaction

= 3 × 2 × 10⁻⁴

= 6 × 10⁻⁴ mol L⁻¹ s⁻¹