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If I recall correctly I was told that the rate of reaction approximately doubled for every 10 degree C rise in temperature. Is the a similar rule of thumb for increase in pressure. I am working on putting a relatively simple explanation for Creationists of how 'chance' could produce complex molecules following the example of the Miller-Urey experiment.

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closed as unclear what you're asking by Mithoron, Mathew Mahindaratne, Todd Minehardt, airhuff, Jan Jan 13 at 15:19

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  • $\begingroup$ Related: Clausius-Clapeyron relation $\endgroup$ – Eashaan Godbole Jan 12 at 11:35
  • $\begingroup$ @EashaanGodbole how is Clausius-Clapeyron relation "related" to the question is unclear for me. The question is clearly about chemical kinetics, and Clausius-Clapeyron is all about the phase transitions in chemical thermodynamics. $\endgroup$ – voffch Jan 12 at 12:43
  • $\begingroup$ @voffch The question, referencing the relationship between rate and temperature which is like $\ln{k}\propto\dfrac{1}{T}$, asks about pressure and temperature. As "which" pressure isn't mentioned, I suggested the Clausius-Clapeyron relation which gives $\dfrac{dP}{dT}\propto\dfrac{1}{T^2}$ for vapour pressure vs temperature. $\endgroup$ – Eashaan Godbole Jan 13 at 21:36
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If you're looking for an intuitive explanation, it usually goes as follows: for a reaction between several molecules to occur, they must "hit" each other. Higher temperature means that molecules move more rapidly, colliding with each other more frequently, hence the increase in reaction rates. Higher pressure means that the concentrations of molecules are higher, elevating the collision probability, resulting in an increase of reaction rates. Mathematically, Rate Equation, $v = k[\ce{A}]^x[\ce{B}]^y...$, is perhaps the first equation students learn in kinetics - reaction rate is directly proportional to the constant $k$ multiplied by the concentrations of reactants ($[\ce{A}]$, $[\ce{B}]$) in some exponents ($x$, $y$).

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