Question

Consider the following reaction, the rate expression of which is given below

A + B → C

\(rate = k [A]^{1/2} [B]^{1/2}\)

The reaction is initiated by taking 1M concentration A and B each. If the rate constant (k) is \(4.6 \times 10 ^{-2} \,s^{-1},\) then the time taken for A to become 0.1 M is____sec. (nearest integer)

Answer 1

Correct answer is : 50

\(K =\frac {2.303}{t}\log \frac {1}{0.1}\)

\(4.6 \times 10 ^{-2} = \frac {2.303}{t}\)

t = 50 sec.