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Consider the following reversible reaction,The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in J mol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of Gθ (in J mol−1) for the reaction at 300 K is ____.(Given; ln (2) = 0.7, RT = 2500 J mol−1 at 300 K and G is the Gibbs energy)Correct answer is '8500'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Consider the following reversible reaction,The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in J mol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of Gθ (in J mol−1) for the reaction at 300 K is ____.(Given; ln (2) = 0.7, RT = 2500 J mol−1 at 300 K and G is the Gibbs energy)Correct answer is '8500'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Consider the following reversible reaction,The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in J mol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of Gθ (in J mol−1) for the reaction at 300 K is ____.(Given; ln (2) = 0.7, RT = 2500 J mol−1 at 300 K and G is the Gibbs energy)Correct answer is '8500'. Can you explain this answer?.

Solutions for Consider the following reversible reaction,The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in J mol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of Gθ (in J mol−1) for the reaction at 300 K is ____.(Given; ln (2) = 0.7, RT = 2500 J mol−1 at 300 K and G is the Gibbs energy)Correct answer is '8500'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE. Download more important topics, notes, lectures and mock test series for JEE Exam by signing up for free.

Here you can find the meaning of Consider the following reversible reaction,The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in J mol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of Gθ (in J mol−1) for the reaction at 300 K is ____.(Given; ln (2) = 0.7, RT = 2500 J mol−1 at 300 K and G is the Gibbs energy)Correct answer is '8500'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of Consider the following reversible reaction,The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in J mol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of Gθ (in J mol−1) for the reaction at 300 K is ____.(Given; ln (2) = 0.7, RT = 2500 J mol−1 at 300 K and G is the Gibbs energy)Correct answer is '8500'. Can you explain this answer?, a detailed solution for Consider the following reversible reaction,The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in J mol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of Gθ (in J mol−1) for the reaction at 300 K is ____.(Given; ln (2) = 0.7, RT = 2500 J mol−1 at 300 K and G is the Gibbs energy)Correct answer is '8500'. Can you explain this answer? has been provided alongside types of Consider the following reversible reaction,The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in J mol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of Gθ (in J mol−1) for the reaction at 300 K is ____.(Given; ln (2) = 0.7, RT = 2500 J mol−1 at 300 K and G is the Gibbs energy)Correct answer is '8500'. Can you explain this answer? theory, EduRev gives you an ample number of questions to practice Consider the following reversible reaction,The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (in J mol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of Gθ (in J mol−1) for the reaction at 300 K is ____.(Given; ln (2) = 0.7, RT = 2500 J mol−1 at 300 K and G is the Gibbs energy)Correct answer is '8500'. Can you explain this answer? tests, examples and also practice JEE tests.