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?

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?
Answer
Given that
k = 2.5 × 10⁻⁴ mol⁻¹ L 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 × 10⁻⁴ mol L^-1 s⁻¹
Rate of production of H₂ = 3k = 3 x 2.5 × 10⁻⁴ mol L^-1 s⁻¹ = 7.5 × 10⁻⁴ mol L^-1 s⁻¹