Which of these does not influence the rate of reaction?
Nature of the reactants
Concentration of the reactants
Temperature of the reaction
Molecularity of the reaction
Additional Questions
|
The rate constants 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 |
Answer |
|
Units of rate constant of first and zero order reactions in terms of molarity M unit are respectively |
Answer |
|
If 60% of a first order reaction was completed in 60 minutes, 50% of the same reaction would be completed in approximately |
Answer |
|
In a first order reaction A → B, if k is rate constant and initial concentration of the reactant A is 0.5 M, then the half–life is |
Answer |
|
Consider the reaction: N2(g) + 3H2(g) → 2NH3(g) The equality relationship between $\dfrac{\text{d}[NH_3]}{\text{d}t}$ and $\dfrac{\text{d}[H_2]}{\text{d}t}$ is |
Answer |
|
For the reaction: 2A + B → 3C + D, which of the following does not express the reaction rate? |
Answer |
|
The energies of activation for forward and reverse reactions for A2 + B2 ⇌ 2AB are 180 kJ mol–1 and 200 kJ mol–1 respectively. The presence of a catalyst lowers the activation energy of both (forward and reverse) reactions by 100 kJ mol–1. The enthalpy change of the reaction (A2 + B2 → 2AB) in the presence of catalyst will be (in kJ mol–1): |
Answer |
|
Rate of a reaction can be expressed by Arrhenius equation as: k = Ae–E/RT In this equation, E represents |
Answer |
|
In a first order reaction, the concentration of the reactant decreases from 0.8 M to 0.4 M in 15 minutes. The time taken for the concentration to change from 0.1 M to 0.025 M is |
Answer |
|
For the reaction, N2 + 3H2 → 2NH3, if $\dfrac{\text{d}NH_3}{\text{d}t}$ = 2 × 10–4 mol L–1 s–1, the value of –$\dfrac{\text{d}H_2}{\text{d}t}$ would be |
Answer |