For a first order reaction A ⟶ B the reaction rate at reactant concentration of 0.01 M is found to be 2.0 × 10^-5 mol L^-1 s^-1. The half life period of the reaction is

30 s
220 s
300 s
347 s

Solution

The rate of a first order reaction is 1.5 × 10^-2 mol L^-1 min^-1 at 0.5 M concentration of the reactant. The half life of the reaction is

0.383 min
23.1 min
8.73 min
7.53 min

Solution

Out of the following reaction which will proceed in forward direction if volume of container is increased?

H₂ + Cl₂ ⟶ 2HCl
CaCO₃ ⟶ CaO + CO₂
N₂ + 3H₂ 2NH₃
N₂ + 2O₂ ⟶ N₂O₄

Solution

CaCO₃ ⟶ CaO + CO₂
This reaction will proceed in forward direction if volume of container is increased.

The reaction A ⟶ B follows first order kinetics. The time taken for 0.8 mole of A to produce 0.6 mole of B is 1 hour.What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of B?

2 hours
1 hour
0.5 hour
0.25 hour

Solution

A first order reaction is 50% completed in 30 minutes at 27ºC.Its rate constant is :

2.31 × 10^-2 minute^-1
3.21 × 10^-5 minute^-1
4.75 × 10^-2 minute^-1
1.33 × 10^-3 minute^-1

Solution

3A ⟶ B + C, it would be a zero order reaction when

the rate of reaction is proportional to square of concentration of A
the rate of reaction remains same at any concentration of A
the rate remains unchanged at any concentration of Band C
the rate of reaction doubles if concentration of B is increased to double

Solution

For reaction 3A ⟶ B + C
If it is zero order reaction r= k=[A]⁰, i.e., the rate remains same at any concentration of 'A'. i.e., independent of concentration of A.

Half life of a first order reaction is 4s and the initial concentration of the reactant is 0.12 M. The concentration of the reactant left after 16 s is

0.0075 M
0.06 M
0.03 M
0.015 M

Solution

The plot of concentration of the reactant vs time fora reaction is a straight line with a negative slope. The reaction follows a rate equation

zero order
first order
second order
third order

Solution

After how many seconds will the concentration of the reactants in a first order reaction be halved, if the decay constant is 1.155 × 10^-3 sec^-1.

Solution

A substance’A’ decomposes by a first order reaction starting initially with[A] = 2.00 M and after 200 min, [A] becomes 0.15 M.For this reaction t_1/2 is

53.72 min
50.49 min
48.45 min
46.45 min

Solution

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