The accompanying graph shows plots of ln k versus 1>T for two different reactions. The plots have been extrapolated to the y-intercepts. Which reaction (red or blue) has (a) the larger value for Ea,

Video transcript

Hi everyone. This problem reads the following graph is an Iranian plot for two different chemical reactions marked reaction one and reaction to identify which one of the two reactions has a smaller value of the activation energy. Okay, so this is what we want to determine here. And we know we have an Iranian plot. So let's go ahead and write out our Iranian equation and linear form. And when we write that out it is Ln of K. Is equal to negative activation energy over gas constant R times one over temperature plus Ln. Of a. So with this Iranian equation we can compare this equation to the equation for a straight line which is Y equals M X plus B. Now let's remember that the Iranian equation shows the relationship between temperature. Okay. And the rate constant K. Alright, so with our equation for a straight line we see that M is equal to the slope of the line and that is equal to negative activation energy over our Okay, so let's write that out. So M is equal to negative activation energy over our we're comparing our equation for a straight line to our Iranians equation in linear form. So looking at our two reactions reaction one and reaction to reaction one has a smaller value of the slope. Okay, so because it has a smaller value of the slope, the value of the activation energy should be smaller for reaction one. Alright, so out of the two reactions the one that has the smaller value of the activation energy is going to be reaction one. So let's go ahead and highlight that here. Alright, so Its reaction one because it has the smaller value of the slope. That's it for this problem. I hope it was helpful.