[A] v. Time
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[A] v. Time
For a first order reaction the [A] v Time plot is a decreasing exponential but what would the graph of [A] v Time look like for a second order reaction?
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Re: [A] v. Time
The graph of 1/[A] v Time for a second-order reaction yields a line with slope=k and y-intercept=1/[A]i. Hence the graph of [A] v Time for a second-order reaction would not be linear. The graph would be a rational function with a vertical asymptote at t= -1/(k[A]i).
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Re: [A] v. Time
If you look at the graoh of 1/[A] v Time for a second-order reaction, the slope is equal to K. The y intercept =1/[A]i. This means the graph for a second order reaction would be linear.
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Re: [A] v. Time
The graph of [A] vs time would not be linear for a second order reaction. It is only linear for zero order. For second order the graph of 1/[A] vs t is a linear function with a slope equivalen to +k.
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Re: [A] v. Time
I believe that the second order would be a linear function (straight line) with a positive slope of +k. The graph would be 1/[A]. Hope that helps!
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Re: [A] v. Time
ln[A] vs time will be a straight line for first order reactions and [A] vs time will be a straight line for zero order reactions.
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Re: [A] v. Time
[A] vs time for a second order reaction would look like a steeper exponential function than a decreasing exponential, it could only be linear if it was 1/[A] vs time. If you have a graphing calculator and graph 1/X it would look similar to that.
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Re: [A] v. Time
For a second order reaction, the graph of 1/[A] (not [A]) vs time would be linear with a slope = k.
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Re: [A] v. Time
Hi,
The plot of a second-order reaction would be a linear (straight line) graph with a positive slope of K+.
The plot of a second-order reaction would be a linear (straight line) graph with a positive slope of K+.
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Re: [A] v. Time
Second order reactions when plotted 1/[A] vs time will be an increasing linear graph. k will be the slope of this line.
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