Question 12 of 37intermediate🔧 ApplyNumerical2 marks

The decomposition of NH3\text{NH}_3 on platinum surface is zero order reaction. What are the rates of production of N2\text{N}_2 and H2\text{H}_2 if k=2.5×10−4 mol−1 L s−1k = 2.5 \times 10^{-4} \text{ mol}^{-1} \text{ L s}^{-1}?

Correct Answer

Rate of production of N₂ = 2.5×102.5 \times 10⁻⁴ mol L⁻¹ s⁻¹ Rate of production of H₂ = 7.5×107.5 \times 10⁻⁴ mol L⁻¹ s⁻¹

Exercise: EXERCISES | Q: 3.3 | (Page 25)
For More Understanding

Explanation

For a zero order reaction, the rate is independent of reactant concentration and equals the rate constant k. From the balanced equation 2NH₃ → N₂ + 3H₂, we use stoichiometric coefficients to relate the rates of product formation to the reaction rate.

Solution Steps

  1. Step 1: Write the balanced chemical equation: 2NH₃(g) → N₂(g) + 3H₂(g)

  2. Step 2: For zero order reaction, Rate = k[NH₃]⁰ = k = 2.5×102.5 \times 10⁻⁴ mol L⁻¹ s⁻¹

  3. Step 3: Rate of production of N₂ = d[N₂]/dt = Rate = k = 2.5×102.5 \times 10⁻⁴ mol L⁻¹ s⁻¹

  4. Step 4: Rate of production of H₂ = d[H₂]/dt = 3 × Rate = 3k = 3×2.53 \times 2.5 × 10⁻⁴ = 7.5×107.5 \times 10⁻⁴ mol L⁻¹ s⁻¹

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