JEE Advanced 2016Paper 1
- Exam
- JEE Advanced
- Year
- 2016
- Paper
- Paper 1
- Subject
- Chemistry
- Chapter
- Chemical Kinetics
JEE Advanced 2016 · Paper 1 · Chemistry · Chemical Kinetics
According to the Arrhenius equation,
According to the Arrhenius equation,
Options
- AA high activation energy usually implies a fast reaction
- BRate constant increase with increase in temperature. This is due to a greater number of collisions whose energy exceeds the activation energy
- CHigher the magnitude of activation energy, stronger is the temperature dependence of the rate constant
- DThe pre-exponential factor is a measure of the rate at which collisions occur, irrespective of their energy.
Correct answer
B. Rate constant increase with increase in temperature. This is due to a greater number of collisions whose energy exceeds the activation energy
Step-by-step solution
A]
High means less k, hence slower rate.
B] = fraction of molecules having kinetic energy greater than activation energy which increase as temperature increases.
C] ln \left[\dfrac{1}{{T}_{1}} - \dfrac{1}{{T}_{2}}\right]\dfrac{{K}_{2}}{{k}_{1}} ∝ {E}_{a}∝∝ {Z}_{AB} \times \left(P \times {e}^{- {E}_{a} / RT}\right)∝ A{e}^{- {E}_{a} / RT}
High means less k, hence slower rate.
B] = fraction of molecules having kinetic energy greater than activation energy which increase as temperature increases.
C] ln \left[\dfrac{1}{{T}_{1}} - \dfrac{1}{{T}_{2}}\right]\dfrac{{K}_{2}}{{k}_{1}} ∝ {E}_{a}∝∝ {Z}_{AB} \times \left(P \times {e}^{- {E}_{a} / RT}\right)∝ A{e}^{- {E}_{a} / RT}