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?

k = 2.5 × 10⁻⁴mol⁻¹L s⁻¹
Order of reaction = 0
Decomposition reaction of NH₃
Here NH3 has 2 mol then N₂ and H₂ has 1 and 3 moles respectively
Use the formula of rate of reaction
Use this formula we get
Another formula of rate, Rate = k[NH₃]^x
Given that order of reaction x = 0
Plug the values we get
Plug the value of k we get
Rate of production of N₂= k = 2.5 × 10⁻⁴mol L^-1s⁻¹
Rate of production of H₂= 3k = 3 x 2.5 × 10⁻⁴mol L^-1s⁻¹= 7.5 × 10⁻⁴mol L^-1s⁻¹