The decomposition of N ₂ O _ 5(g) occurs as: 2 N ₂ O _ 5(g) 4 NO _ 2(g) + O _ 2(g) . If initial concentration of N ₂ O _ 5(g) is 1.63 10⁻² mol L ⁻¹ and after 400 seconds it is 1.36 10⁻² mol L ⁻¹ , calculate the rate of reaction.

Step-by-step solution

The rate of reaction is given by the expression: Rate = - 1 2 [ N ₂ O ₅] t [ N ₂ O ₅] = 1.36 10⁻² - 1.63 10⁻² = -0.27 10⁻² mol L ⁻¹ t = 400 s Rate = - 1 2 ( -0.27 10⁻² 400 ) Rate = 0.27 10⁻² 800 = 3.375 10⁻⁶ mol L ⁻¹ s ⁻¹ Rounding off, the rate of reaction is 3.38 10⁻⁶ mol L ⁻¹ s ⁻¹ . Answer: 3.38 10⁻⁶ mol L ⁻¹ s ⁻¹