Reaction A + B → C + D follows rate law R = K[A] 1/2 [B] 1/2 starting with 1 M of A and B. What is time taken for concentration of A to become 0.1 M ? [Given, K = 4.606 x 10 -4 s -1 ]

Step-by-step solution

R = K A 1 / 2 B 1 / 2 dx dt = K 1 - x 1 / 2 1 - x 1 / 2 dx dt = K 1 - x Integrating on both sides K = 2.303 t log 1 1 - x , ( ∴ ( 1 - x ) = 0 . 1 M at time t ) ⇒ 4.606 × 1 0 - 4 = 2.303 t log 1 0.1 = 2.303 t ⇒ 2 × 1 0 - 4 = 1 t or t = 1 0 4 2 = 1 0 0 0 0 2 = 5000 s