Good day! I have a question from my chem HW that is stumping me. Although the answer may be simple, it has eluded me for quite a bit. It regards rate laws and constants of reactions.
Question is as stated: This reaction was monitored as a function of time: AB --> A + B
A plot of 1/[AB] versus time yields a straight line
with slope= - 0.055 M-1s-1
What is the value of the rate constant (k) at this temp?
SINCE it stated 1/[AB] vs. time, its implying an order 2 reaction since order 2 reaction
has the integrated rate law:
1/[AB]t = kt + 1/[AB]0
y axis = 1/[AB].......
The Attempt at a Solution
When a order 2 reaction is plotted against time, k = slope. When the question stated it was talking about a plot of 1/[AB] its referring to a order 2 reaction, and since order 2 reactions (when plotted against time) have a y axis = 1/[AB], im deducing the reaction is order 2.
I'm confused since the given slope is negative, and every graph of an order 2 reaction vs. time in my book has a straight line with a positive slope.
Like I said, its an easy problem, with an easy solution, but i'm not seeing it.