The rate of reactions proportional to square of concentration of A.
The rate of reaction remains same at any concentration of A.
The rate remains uncharged at any concentration of B and C
The rate of reaction doubles if concentration of b is increased to double.
The plot of concentration of the reactant vs time for a reaction is a straight line with a negative slope.This reaction follows.
Zero order rate equation.
First order rate equation.
Second order rate equation.
Third order rate equation.
The reaction follows first order kinetics. The time taken for 0.8 mole of A to produce 0.6 mole of B 1 h. What is the time taken for the conversion of 0.9 mole of A to 0.675 mole of B ?
0.25 h
2 h
1 h
0.5 h
The reaction of hydrogen and iodine monochloride is given as.
B only
A and B both
Neither A nor B
A only
For a first order reaction the reaction rate at reactant concentration of 0.01 M is found to be 2.0 x 10-5 ,mol L-1 s-1. The half-life period of the reaction is.
220 s
30 s
300 s
347 s
For exothermic reaction, the energy of activation is.
Equal to the energy of activation of products.
Less than the energy of activation of product.
Greater than the energy of activation of products.
sometimes greater and sometimes less than that of the products.
In a reversible reaction,the energy of activation of the forward reaction is 50 kcal. The energy of activation for the reverse reaction will be.
< 50 kcal
50 kcal
Either greater than or less than 50 kcal.
> 50 kcal
The rate constant k1 and k2 for two different reactions are 1016.e-2000/T and 1015.e-1000/T, respectively. The temperature at which k1 =k2 is
1000 k
2000 k
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.
