00:01
To determine the rate constant at a different temperature, we'll be using a form of the arrhenius equation, where the natural log of the rate constant at a higher temperature divided by the rate constant at a lower temperature equals negative activation energy divided by the constant r multiplied by 1 over t2 minus 1 over t1.
00:23
So we'll take the natural log of the ratio of the rate constants, the higher temperature divided by the lower temperature, set that equal to negative ea in units of joules per mole, so positive 107 kilojoules per mole is 107 ,000 joules per mole, and then we'll include the negative sign.
00:42
We'll divide by r, the constant 8 .314 joules per kelvin mole, then multiply by 1 over t2, which is what we want to determine, the temperature at which the rate constant is this value, minus 1 over t1.
00:56
When using this equation, temperatures need to be in kelvin, so we'll add 273 to the celsius value to get it into kelvin.
01:05
The natural log of the ratio is 1 .010...