The experimental data for the reaction
The rate of reaction between two reactants A and B decreases by a factor of 4, if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is.
-1
-2
1
2
For the reaction,Products, it is observed that.
Rate = k[A2[B]
Rate = k[A][B]2
Rate = k[A]2[B]2
Rate = k[A][B]
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.
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
If the rate of a reaction is equal to the rate constant, the order of the reaction is.
3
0
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
In the following reaction, how is the rate of appearance of the underlined product related to the rate of disappearance of the underlined reactant?
