**Question 16**A chemical reaction has a specific-rate constant \(1.10 \times 10^{-4}\text{ s}^{-1}\) at 470°C. At what temperature will the rate constant equal \(4.36 \times 10^{-3}\text{ s}^{-1}\), if the activation energy is 264 kJ/mol?- [ ] 540°C- [ ] 510°C- [ ] 411°C- [ ] 126°C**Explanation of Answer Choices:**- \(540°C\)- \(510°C\)- \(411°C\)- \(126°C\)This question is related to calculating the temperature at which the rate constant of a chemical reaction changes, given its specific-rate constant at a known temperature and the activation energy. The Arrhenius equation (\(k = A \exp(-E_a / RT)\)) is typically used to solve this kind of problem, where \(k\) is the rate constant, \(E_a\) is the activation energy, \(R\) is the gas constant, and \(T\) is the temperature in Kelvin.

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Answered: D Question 16 An chemical reaction has…

D Question 16 An chemical reaction has specific-rate constant 1.10 x 104s¹ at 470 C. At what temperature will the rate constant equal 4.36 x 10-³ s¹¹, if the activation energy is 264 kJ/mol?

Chemistry

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ISBN:9781305957404

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Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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