Reaction `A+B rarr 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=4.606xx10^(-4)s^(-1)` ]

Reaction A+BrarrC+D follows rate law . r=k[A]^(1//2)[B]^(1//2) Starting with 1 M of A and B each. What is the time taken fro concetration of A become 0.1M ? (Given k=2.303xx10^(-2)sec^(-1))

Reaction A+BrarrC+D follows rate law . r=k[A]^(1//2)[B]^(1//2) Starting with 1 M of A and B each. What is the time taken fro concetration of A become 0.1M ? (Given k=2.303xx10^(-2)sec^(-1))

Reaction A+BrarrC+D follows rate law . r=k[A]^(1//2)[B]^(1//2) Starting with 1 M of A and B each. What is the time taken fro concetration of A become 0.1M ? (Given k=2.303xx10^(-2)sec^(-1)) a) 10 sec b) 100 sec c) 1000 sec d) 434 sec

Reaction A + B rarr C + D follows rate law, r = k[A]^(1//2) [B]^(1//2) starting with 1 MofA and Beach. What is the time taken for concentration of A become 0.1 M? (K = 2.303 * 10 ^(-3) )

Reaction A+BtoC+D is started with 1 M of each A and B and follows the rate law r=k[A]^(1//2)[B]^(1//2) What is the time taken for the concentration of A to drop to 0.1 M (K=2.303xx10^(-3)sec^(-1))

For a reaction A+B to P, the rate law is given by: r=k[A]^(1//2)[B]^(2) What is the order of the reaction?

For a reaction having rate law expression : Rate = k[A]^(3//2) [B]^(-1//2) If the concentration of both A and B become four times the rate of reaction