For a first-order reaction A \(\rightarrow\) Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in min^-1 is

The rate constant for a first order reaction is $4.606\times {10}^{-3} s^{-1}$. The time required to reduce 2.0 g of the reactant to 0.2 g is:

If the rate constant for a first order reaction is k, the time (t) required for the completion of 99% of the reaction is given by:

1. t=2.303/k

2. t=0.693/k

3. t=6.909/k

4. t=4.606/k

A first-order reaction has a rate constant of 2.303$\times {10}^{-3}$ ${\mathrm{s}}^{-1}$. The time required for 40 g of this reactant to reduce to 10 g will be [Given that ${\log }_{10}2=0.3010$]

1. 230.3 s

2. 301 s

3. 2000 s

4. 602 s

A first-order reaction has a specific reaction rate of
10^-2 sec^-1. How much time will it take for 20 g of the reactant to reduce to 5 g?

In a zero-order reaction for every 10 ° rise of temperature, the rate is doubled.
If the temperature is increased from 10 °C to 100 °C,
the rate of the reaction will become:

1. 256 times

2. 512 times

3. 64 times

4. 128 times

The half-life of a certain enzyme catalysed reaction is 138 s, that follow the 1st order kinetics. The time required for the concentration of the substance to fall from 1.28 mg L^–1 to 0.04 mg L^–1, is:

1. 276 s 

2. 414 s

3. 552 s 

4. 690 s

The reaction of hydrogen and iodine monochloride is given as: 
H₂(g) + 2ICl(g) → 2HCl(g) + I₂(g) 
This reaction is of first order with respect to H₂(g) and ICl(g), for which of the following proposed mechanisms:
Mechanism A: 
H₂(g) + 2ICl(g) → 2HCl(g) + I₂(g) 
Mechanism B: 
H₂(g) + ICl(g) →HCl(g) + HI(g); slow 
HI(g) + ICl(g) →HCl(g) + I₂(g); fast

1. B Only

2. A and B both

3. Neither A nor B

4. A only