In a reaction, 2 N ₂ O _ 5(g) 4 , NO _ 2(g) + O _ 2(g) N ₂ O ₅ disappears at a rate of 0.06 mol dm ⁻³ s ⁻¹ Calculate rate of formation of O _ 2(g) ?

Step-by-step solution

For the given reaction 2 N ₂ O _ 5(g) 4 NO _ 2(g) + O _ 2(g) The rate of reaction is given by: Rate = - 1 2 d[ N ₂ O ₅] dt = 1 4 d[ NO ₂] dt = d[ O ₂] dt Given the rate of disappearance of N ₂ O ₅ is - d[ N ₂ O ₅] dt = 0.06 mol dm ⁻³ s ⁻¹ The rate of formation of O ₂ is: d[ O ₂] dt = 1 2 (- d[ N ₂ O ₅] dt ) d[ O ₂] dt = 1 2 0.06 = 0.03 mol dm ⁻³ s ⁻¹