NEET

Half life period of a first-order reaction is 1386 seconds. The specific rate constant of the reaction is :

0.5 × 10^-2 s^-1
0.5 × 10^-3 s^-1
5.0 × 10^-2 s^-1
5.0 × 10^-3 s^-1

Solution

Solution

Solution

Solution

In a first-order reaction A ⟶ B, if k is rate constant and inital concentration of the reactant A is 0.5 M, then the half-life is

\(\frac{log2}{k}\)
\(\frac{log2}{k\sqrt{0.5}}\)
\(\frac{ln 2}{k}\)
\(\frac{0.693}{0.5k}\)

Solution

A and B both
neither A nor B
A only
B only

Solution

As the slowest step is the rate determining step thus the mechanism B will be more consistent with the given information also because it involve one molecule of H₂ and one molecule of ICl it can expressed as r = k[H₂][ICl]Which shows that the reaction is first order w.r.t. both H₂ & ICl.

In a first order reaction, the concentration of the reactant is reduced to 18 of the initial concentration in 75 minutes at 298 K. What is the half-life period of the reaction in minutes?

Solution

When a biochemical reaction is carried out in laboratory in the absence of enzyme then rate of reaction obtained is 10^–6 times, then activation energy of reaction in the presence of enzyme is