In the following reaction, how is the rate of appearance of the underlined product related to the rate of disappearance of the underlined reactant?
The temperature dependance of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, k = Ae-E*/RT. Activation energy (E*) of the reaction can be calculated by plotting
log k vs 1/T
k vs T
A chemical reaction is catalysed by a catalyst X. Hence, X
Reduces enthalpy of the reaction
Decreases rate constant of the reaction
Increases activation energy of the reaction
Does not affect equilibrium constant of the reaction
The rate of 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
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
The representation of rate of reaction in terms of concentration of the reactants is known as ______________
partial pressure
rate law
average rate
total rate
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 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.
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
For the reaction 2N2O5 → 4NO2 + O2, rate and rate constant are 1.02 × 10-4 and 3.4 × 10-5 s -1 respectively, then concentration of N2O5 at that time will be
1.732
3
1.02 × 10-4
3.4 × 105
