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If the rate constant doubles, for example, so also will the rate of the reaction. You can use the Arrhenius equation to show the effect of a change of temperature on the rate constant - and therefore on the rate of the reaction. If you need to use this equation, just find the "ln" button on your calculator. You may also come across it in a different form created by a mathematical operation on the standard one: It is often taken as constant across small temperature ranges.īy this time you've probably forgotten what the original Arrhenius equation looked like! Here it is again: It varies slightly with temperature, although not much.
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You may also find this called the pre-exponential factor.Ī is a term which includes factors like the frequency of collisions and their orientation. You will find a simple calculation associated with this further down the page. You should find an e x button - probably on the same key as "ln".įor reasons that are beyond the scope of any course at this level, this expression counts the fraction of the molecules present in a gas which have energies equal to or in excess of activation energy at a particular temperature. You don't need to worry exactly what it means, although if you have to do calculations with the Arrhenius equation, you may have to find it on your calculator. and is a mathematical number, a bit like pi. Use the BACK button on your browser to return to this page. Introductory page on rates of reaction before you go on. Note: If you aren't sure about activation energy, you should read the To fit this into the equation, it has to be expressed in joules per mole - not in kJ mol -1. This is the minimum energy needed for the reaction to occur. It turns up in all sorts of unlikely places! This is a constant which comes from an equation, pV=nRT, which relates the pressure, volume and temperature of a particular number of moles of gas. To fit into the equation, this has to be meaured in kelvin. This is shown mathematically in the Arrhenius equation. If you change the temperature or the catalyst, for example, the rate constant changes. These are all included in the so-called rate constant - which is only actually constant if all you are changing is the concentration of the reactants. What about all the other things (like temperature and catalysts, for example) which also change rates of reaction? Where do these fit into this equation? The rate equation shows the effect of changing the concentrations of the reactants on the rate of the reaction.
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Note: If you don't remember this, you must read the page about orders of reaction before you go on. You will remember that the rate equation for a reaction between two substances A and B looks like this: If you aren't reasonably confident about the basic rates of reaction work, explore the rates of reaction menu first. This present page is at the hard end of the rates of reaction work on this site. Note: If you aren't sure what a rate constant is, you should read the page about orders of reaction before you go on. This page looks at the way that rate constants vary with temperature and activation energy as shown by the Arrhenius equation. RATE CONSTANTS AND THE ARRHENIUS EQUATION Rate constants and the arrhenius equation