The rate law for the chemical reaction 2NO2Cl → 2NO2 + Cl2 is Rate = k [NO2Cl]. The rate determining step is
2NO2Cl → 2NO2 + 2Cl
NO2 + Cl2 → NO2Cl + Cl
NO2Cl + Cl → NO2 + Cl2
NO2Cl → NO2 + Cl
The correct statement is
The rate constant of an exothermic reaction decreases with increase in temperature
The rate constant of an endothermic reaction increases with increase in temperature
The rate constant of forward and backward directions of a reversible reaction decreases with increase in temperature
The rate constant of forward direction increases while that of backward reaction decreases with increase in temperature.
In the case of a first order reaction, when log k (y-axis) is plotted against 1/T, a straight line graph with slope -1.25×104 is obtained. The energy of activation for the reaction is
28.78 kJ mol-1
2.77 kJ mol-1
239.34 kJ mol-1
27.7 kJ mol-1
The rate equation for a reaction is r = k[A]n. The rate of the reaction remains unchanged on reducing the volume of the reaction vessel to half the initial value. The order of the reaction is
1
2
0
3
In the first order reaction
Rate constant is independent of initial concentration
Half life is independent of rate constant
Half lives of liquid state reactions are more than those of gas phase reactions
Half life is independent of activation energy
A hypothetical reaction 2p + q → s + r has rate constant as 2.0 × 10-3 mol L-1 s-1. The order of the reaction is
Unpredictable
Zero
One
Two
The rate constants k1 and k2 for two different reaction 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 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
The incorrect statements is
The average speed of a reaction decreases with time
For the reaction A = 2B, the rate of disappearance of concentration of B and rate of reaction represent one and the same thing
For a reaction, 2N2(g) + 3H2(g) → 2NH3(g), the rate law is given as - ½ d[N2]/dt
The unit of rate constant for zero order reaction is mol dm-3 s-1
