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The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol⁻¹.The ratio of rate constant to the Arrhenius factor is
Options
(a) 0.01
(b) 0.1
(c) 0.02
(d) 0.001
Correct Answer:
0.1
Explanation:
Arrhenius equation K=A.e(-Eₐ/RT)
⇒In K =In A -Eₐ/RT slop = -Eₐ/R
so,activation energy of reaction can be determined from the slop of In K vs 1/T
Related Questions: - 1.0g of magnesium is burnt with 0.56 g O₂ in a closed vessel
- The first ionisation potential will be maximum for
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Topics: Electrochemistry and Chemical Kinetics
(87)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- 1.0g of magnesium is burnt with 0.56 g O₂ in a closed vessel
- The first ionisation potential will be maximum for
- Electric configuration of chalcogens in their outermost orbit is
- Least voltage hydrogen halide is
- In SN2 reaction the sequence of bond breaking and bond formation is as follows
Topics: Electrochemistry and Chemical Kinetics (87)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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