Reaction A + B longrightarrow C + D follows following rate law: rate = k [ A ]+(1/2)[ B ](1/2). Starting with initial conc. of 1 M of A and B each, what is the time taken for concentration of A become 0.25 M. Given: k =2.303 × 10-3 sec -1.

Question

Reaction A + B longrightarrow C + D follows following rate law: rate = k [ A ]+(1/2)[ B ](1/2). Starting with initial conc. of 1 M of A and B each, what is the time taken for concentration of A become 0.25 M. Given: k =2.303 × 10-3 sec -1. (A) 300 s (B) 600 s (C) 900 s (D) 1200 s

Tardigrade Admin · Accepted Answer

It is a first order reaction t =(2.303/2.303 × 10-3) log (1/0.25) t =1000 × 0.6=600 second

Q. Reaction $A + B ⟶ C + D$ follows following rate law : rate $= k [A]^{+ \frac{1}{2}} [B]^{\frac{1}{2}}$ . Starting with initial conc. of $1 M$ of $A$ and $B$ each, what is the time taken for concentration of A become $0.25 M$ . Given : $k = 2.303 \times 1 0^{- 3} se c^{- 1}$ .

300 s

600 s

900 s

1200 s

It is a first order reaction
$t = \frac{2.303}{2.303 \times 1 0 ^{- 3}} lo g \frac{1}{0.25}$
$t = 1000 \times 0.6 = 600$ second

Q. Reaction A+B⟶C+D follows following rate law : rate =k[A]+21​[B]21​. Starting with initial conc. of 1M of A and B each, what is the time taken for concentration of A become 0.25M. Given : k=2.303×10−3sec−1.