Question

In a reaction \[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\], if the rate of disappearance of N_2(g) is 2.6 × 10⁻⁴ M/s, the rate of disappearance of H_2(g) in M/s is ____________.

Options

• 8.6 × 10⁻⁴ M/s

• 5.2 × 10⁻⁴ M/s

• 2.6 × 10⁻⁴ M/s

• 7.8 × 10⁻⁴ M/s

Answer 1

In a reaction \[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\], if the rate of disappearance of N_2(g) is 2.6 × 10⁻⁴ M/s, the rate of disappearance of H_2(g) in M/s is 7.8 × 10⁻⁴ M/s.

Explanation:

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

`-("d"["N"_2])/"dt" = -1/3 ("d"["H"_2])/"dt" = 1/2 ("d"["NH"_3])/"dt"`

`("d"["N"_2])/"dt" = 1/3 ("d"["H"_2])/"dt"`

`2.6 xx 10^-4 = 1/3 ("d"["H"_2])/"dt"`

`("d"["H"_2])/"dt"` = 3 × 2.6 × 10⁻⁴

`("d"["H"_2])/"dt"` = 7.8 × 10⁻⁴ M/s