Question

The decomposition of $\mathrm{NH}_{3}$ on platinum surface is zero order reaction. What are the rates of production of $\mathrm{N}_{2}$ and $\mathrm{H}_{2}$ if $k=2.5 \times 10^{-4} \mathrm{~mol}^{-1} \mathrm{~L} \mathrm{~s}^{-1}$ ?

✨ Free AI Tools for You

Powered by Chatterbot AI

Answer

Rates of Production:

  • Rate of production of (\mathrm{N}_2): [ \text{Rate}_{\mathrm{N}_2} = 1.25 \times 10^{-4} \ \mathrm{mol \ L^{-1} \ s^{-1}} ]

  • Rate of production of (\mathrm{H}_2): [ \text{Rate}_{\mathrm{H}_2} = 3.75 \times 10^{-4} \ \mathrm{mol \ L^{-1} \ s^{-1}} ]

Thus, the rates of production are:

  • $\mathrm{N}_2$: ( \mathbf{1.25 \times 10^{-4} \ \mathrm{mol \ L^{-1} \ s^{-1}}} )

  • $\mathrm{H}_2$: ( \mathbf{3.75 \times 10^{-4} \ \mathrm{mol \ L^{-1} \ s^{-1}}} )


Was this helpful?

India's 1st AI Doubt Solver for CBSE, JEE, and NEET

Ask a Question for Free

and then it's just ₹212 a month