October 09, 2024, 09:08:12 AM
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Topic: Magnesium and hydrochloric acid rate law  (Read 1269 times)

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Offline RandomDude1234

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Magnesium and hydrochloric acid rate law
« on: September 10, 2024, 06:00:25 PM »
Hello, I am trying to determine the activation energy of the magnesium and hydrochloric reaction by measuring the volume of gas produced at different temperatures. In order to to this, I need the rate law (to find the rate constant at different temperatures), however, I have found multiple different rate laws for this reaction. In a worked example from a question in my chemistry textbook it says rate = k(HCl)2, on other online sources/forums, it says rate = k(HCl), and some even include magnesium, or H+ ions into the rate law. If someone could guide me to the correct rate law that would be much appreciated, as I do not have the word count available to include determining the rate law in my lab report. Thank you.

Online mjc123

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Re: Magnesium and hydrochloric acid rate law
« Reply #1 on: September 11, 2024, 09:15:54 AM »
The actual rate law doesn't matter, as long as it is the same across all your experimental conditions. If you use the same HCl concentration in all experiments, then
Rate = constant*e-Ea/RT
and the actual value of constant doesn't matter. Plot log(rate) vs. 1/T.

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