You visited us 2 times! Enjoying our articles? Unlock Full Access!

Redox Reactions

The decomposi...

Question

The decomposition of NH₃ on platinum surface is zero order reaction. What are the rates of production of N₂ and H₂ if k = 2.5 × 10⁻⁴ mol⁻¹ L s⁻¹?

Open in App

Solution

The decomposition of NH₃ on platinum surface is represented by the following equation.

Therefore,

However, it is given that the reaction is of zero order.

Therefore,

Therefore, the rate of production of N₂ is

And, the rate of production of H₂ is

= 7.5 × 10⁻⁴ mol L⁻¹ s⁻¹

Suggest Corrections

Similar questions

N H_{3}

N_{2}

H_{2}

K = 2.5 \times 10^{- 4} m o l l i t r e^{- 1} s^{- 1}

{N H}_{3}

N_{2}

H_{2}

{m o l e . l i t}^{- 1} . {s e c}^{- 1}

K = 2.5 \times 10^{- 4} m o l e . l i t^{- 1} . {s e c}^{- 1}

N H_{3}

N_{2}

H_{2}

(k = 2.5 \times 10^{- 4} m o l L^{- 1} s^{- 1})

N H_{3}

2.5 \times 10^{- 4}

m o l . d m^{- 3}

s^{- 1}

350

4 \times 10^{- 3} m s^{- 1}

N H_{3}

Join BYJU'S Learning Program