The rate constant for the reaction 2 N ₂ O ₅ 4 NO ₂ + O ₂ is 3.0 10⁻⁵ s ⁻¹ . If the rate is 2.4 10⁻⁵ mole L ⁻¹ s ⁻¹ then the concentration of N ₂ O ₅ ,( mol L ⁻¹) is

Step-by-step solution

From the unit of the rate constant ( s ⁻¹ ), we can determine that the given reaction is a first-order reaction. For a first-order reaction, the rate law is expressed as: Rate = k[ N ₂ O ₅] Given values are: Rate = 2.4 10⁻⁵ mole L ⁻¹ s ⁻¹ k = 3.0 10⁻⁵ s ⁻¹ Substituting these values into the rate equation: 2.4 10⁻⁵ = 3.0 10⁻⁵ [ N ₂ O ₅] Solving for the concentration of N ₂ O ₅ : [ N ₂ O ₅] = 2.4 10⁻⁵ 3.0 10⁻⁵ [ N ₂ O ₅] = 2.4 3.0 [ N ₂ O ₅] = 0.8 mol L ⁻¹ Answer: 0.8