16:I[8216,["972","static/chunks/972-b28da0de92681928.js","47","static/chunks/47-a7f06e9eda1ac756.js","115","static/chunks/app/%5Bexam%5D/questions/%5Byear%5D/%5Bsubject%5D/%5Bchapter%5D/%5BquestionId%5D/page-7b6f0a12b9cc0206.js"],"BackButton"] 17:I[1553,["972","static/chunks/972-b28da0de92681928.js","47","static/chunks/47-a7f06e9eda1ac756.js","115","static/chunks/app/%5Bexam%5D/questions/%5Byear%5D/%5Bsubject%5D/%5Bchapter%5D/%5BquestionId%5D/page-7b6f0a12b9cc0206.js"],"QuestionViewer"] 15:T504,{"@context":"https://schema.org","@type":"Quiz","name":"Comedk 2024 Chemical Kinetics PYQ with Solution","url":"https://pyq-test-series-platform-alsjdcxu2-sameers-projects-41c5a71e.vercel.app/comedk/questions/2024/chemistry/chemical-kinetics/lx0kbvie","educationalLevel":"Entrance exam preparation","about":"Comedk / Chemistry / Chemical Kinetics","hasPart":{"@type":"Question","name":"Comedk 2024 Chemical Kinetics PYQ with Solution","text":"The Activation energy for the reaction A \\rightarrow B+C, at a temperature \\mathrm{TK} was 0.04606 \\mathrm{~RT} \\mathrm{~J} / \\mathrm{mol}. What is the ratio of Arrhenius factor to the Rate constant for this reaction?","eduQuestionType":"mcq","acceptedAnswer":{"@type":"Answer","text":"D"},"comment":{"@type":"Comment","text":"The Arrhenius equation is given by: k = A e^{-E_a/RT}, where: k is the rate constant A is the Arrhenius factor or pre-exponential factor E_a is the activation energy R is the ideal gas constant (8.314 J/mol K) T is the temperature in Kelvin. We are given that the activation energy is 0.04606 \\mathrm{~RT} \\mathrm{~J} / \\mathrm{mol} and we need to find the ratio of the Arrhenius factor to the rate constant. This ratio can be obtained by rearranging the Arrhenius equation: A/k = e^{E_a/RT}. Substi..."}}}18:T42c,

The Arrhenius equation is given by:

$$k = A e^{-E_a/RT}$$,

where:

$$k$$ is the rate constant
$$A$$ is the Arrhenius factor or pre-exponential factor
$$E_a$$ is the activation energy
$$R$$ is t

Chemical Kinetics

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