A substance 'A' decomposes by a first order reaction starting initially with [A] = 2.00m and after 200 min, [A] becomes 0.15 m. For this reaction t1/2 is
53.49 min
50.49 min
48.45 min
46.45 min
The order of a reaction with respect of OH- is -1. The OH- species
Act as a catalyst
Act as an inhibitor
Act as a promoter
Always appear in the chemical equation
For exothermic reaction, the energy of activation of the reactants is
Equal to the energy of activation of products
Less than the energy of activation of products.
Greater than the energy of activation of products.
Sometimes greater and sometimes less than that of the products.
In gaseous reactions,the units of the rate equation will be ____________
Mol L-1
mol S-1
atm L-1
atm S-1
For a first-order reaction, the half-life period is independent of
Initial concentration
Cube root of initial concentration
First power of final concentration
Square root of final concentration
For producing effective collisions the colliding molecules must have
A certain minimum amount of energy
Energy equal to or greater than threshold energy
Proper orientation
Both threshold energy and proper orientation
For a chemical reaction , Ea = 0 and the value of rate constant k = 6.8 × 10 -4 at 300 K. The value of ‘k’ if the temperature is doubled is
1.36 × 10-3 s-1
3.4 × 10-4 s-1
6.8 ×10-4 s-1
1.7 × 10-4 s-1
The activation energy for a simple chemical reaction A → B is Eα in forward direction. The activation energy for reverse reaction
Can be less than or more than Eα
Is always double of Eα
Is negative of Eα
Is always less than Eα
Which is a wrong statement?
Order of a reaction is an experimentally determined quantity
Order and molecularity need not be the same for a reaction
Molecularity cannot have fractional values
Molecularity refers to kinetics and order refers to mechanism
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-1s-1. The half-life period of the reaction is
220 s
30 s
300 s
347 s
