Achieve Question #11

[Maritza Jacobo]

Can someone explain how to do the second and third parts of the question? This is what I've been given [N2O5]0=0.0601 mol.L-1 after 1.6h and for my half life I got 5.2. Thank you in advance!

[Maleeha Amir 2E]

So, it's asking what the concentration is after 1.6 hours. Since its a first order reaction, the equation is ln[N2O5] = -kt + ln[N2O5](0). Then you can plug in the values and make sure to convert the time to seconds if your k is in seconds. For the third part, you plug in the final and initial concentrations, k and then solve for t.

[106046096]

Hi! For the other two questions, you would use the integrated rate law for a first-order reaction, which is [A]t = [A]0 e^-kt and plug in the values you have to solve for the missing variables. Also, make sure to convert hours to seconds!

[gary_vernes]

For both of these parts, you will have to use the integrated rate law for a first order reaction, which is [A]t=[A]0e−kt, where [A]t is the concentration at time t and [A]0 is the initial concentration. For the second part of the question, you would solve for [A]t, and for the third part you would rearrange this equation to solve for t(time). Also watch out for the units in the last part, since it's asking you for the time in minutes, not hours.