Kinetics Plots

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Jake Gordon 1A
Posts: 61
Joined: Fri Sep 28, 2018 12:15 am

Kinetics Plots

Postby Jake Gordon 1A » Wed Mar 13, 2019 4:58 pm

I remember that the three plots vs time that we are working with are [A], 1/[A], and ln[A] but what does it mean if we get a straight line for each individual graph?

Nicklas_Wright_1A
Posts: 60
Joined: Fri Sep 28, 2018 12:23 am

Re: Kinetics Plots

Postby Nicklas_Wright_1A » Wed Mar 13, 2019 7:23 pm

A straight line for ln(A) means the reaction is first order. For 1/A it means the reaction is second order. For A it means the reaction is zero order.

Tameen Ahmed 4C
Posts: 30
Joined: Fri Sep 28, 2018 12:19 am

Re: Kinetics Plots

Postby Tameen Ahmed 4C » Wed Mar 13, 2019 8:46 pm

If it's a straight line with a negative slope then it can be zero order or first order. If the graph displays [A] vs. time with a negative slope then it's zero order and if the graph displays ln[A] vs time with a negative slope then it's a first order reaction.

A second order reaction would be plotted as 1/[A] vs. time with a positive slope.

Athena L 1B
Posts: 59
Joined: Fri Sep 28, 2018 12:18 am

Re: Kinetics Plots

Postby Athena L 1B » Thu Mar 14, 2019 11:52 am

If you plot any of those graphs but get a curve, you know you have the wrong order reaction

Henry Dudley 1G
Posts: 61
Joined: Fri Sep 28, 2018 12:16 am

Re: Kinetics Plots

Postby Henry Dudley 1G » Sat Mar 16, 2019 8:42 pm

If the line is straight for a graph, then the reaction is that order. For instance if the data points give you a straight line for lnA on the y-axis and t on the x-axis, you know you have a first order reaction.

105169446
Posts: 32
Joined: Fri Sep 28, 2018 12:16 am

Re: Kinetics Plots

Postby 105169446 » Sun Mar 17, 2019 12:00 am

But if you have a plot of [reactant] vs time for a first order reaction then in that case you'll get an exponential curve which is decreasing.


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