Most of the time, the rate of a reaction depends on the concentration of the reactant. In the case of second-order react

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Most of the time, the rate of a reaction depends on the
concentration of the reactant. In the case of second-order
reactions, the rate is proportional to the square of the
concentration of the reactant.
Select the image to explore the simulation, which will help
you to understand how second-order reactions are identified by the
nature of their plots. You can also observe the rate law for
different reactions.
In the simulation, you can select one of the three different
kinds of plots. You may use
the Start , Stop,
and Reset buttons to observe the
corresponding changes in the plot for different kinds of reactions.
You can also select six different reactions using the drop-down
menu and observe three different types of plots for each
reaction.
Relating plots to the order of a reaction
Consider the following reaction:
A→productsA→products
The plot of [A][A] versus tt is linear for
the zero-order reaction, the plot
of ln[A]ln[A] versus tt is linear for the
first-order reaction, and the plot
of 1[A]1[A] versus tt is linear for the
second-order reaction. [A][A] represents the
concentration of the reactant AA.
The linearity of each graph can be used to identify the order of
a reaction.
Characteristics of second-order reactions
For a second-order reaction, [A]→products[A]→products, the
rate of the reaction is given as rate=rate= k[A]2k[A]2,
where kk is the rate constant and [A][A] is the
concentration of reactant AA. The integrated rate law for
second-order reactions is 1[A]t=kt+1[A]01[A]t=kt+1[A]0,
where [A]t[A]t is the concentration of
reactant AA at time tt, kk is the rate
constant, and [A]0[A]0 is the initial concentration of
reactant AA. This equation is of the type y=mx+by=mx+b.
Therefore, the plot of 1[A]t1[A]t versus time is always a
straight line with a slope kkk and
a yyy intercept 1[A]01[A]0.
Consider the second-order reaction:
2HI(g)→H2(g)+I2(g)2HI(g)→H2(g)+I2(g)
Use the simulation to find the initial
concentration [HI]0[HI]0 and the rate
constant kk for the reaction. What will be the
concentration of HIHI after ttt =
8.20×1010 ss ([HI]t[HI]t) for a reaction
starting under the condition in the simulation?
Express your answer in moles per liters to three significant
figures.
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