00:01
To find the rate constant at the different temperature, we use the arranius equation for the natural log of the rate constant at the different temperature, we'll call it k2, is equal to negative ea, the activation energy, over r multiplied by 1 over the kelvin temperature for which we want to calculate the rate constant, minus 1 over the kelvin temperature for which we know a rate constant, plus the natural log of that known rate constant.
00:33
So the natural log of the rate constant at 314 .4 kelvin is going to be equal to negative activation energy.
00:42
The activation energy is 103 kilojoules per mole, but when using this equation, it must be in joules per mole so that 103 becomes 103 ,000 joules per mole, which we divide by r, 8 .3 .3.
00:59
14 joules per kelvin mole, we multiply by 1 over the kelvin temperature for which we want to figure out the k value, that being 314 .4 kelvin minus 1 over the k value, sorry, the kelvin temperature for which we know a k value, that is 328 kelvin, plus the natural log of the rate constant at 328 kelvin, and that was .0900 inverse minutes...