For a second-order reaction, [A]products, the rate of the reaction is given as r

Question

For a second-order reaction, [A]products, the rate of the reaction is given as rate= k[A]2, where k is the rate constant and [A] is the concentration of reactant A. The integrated rate law for second-order reactions is 1[A]t=kt+1[A]0, where [A]t is the concentration of reactant A at time t, k is the rate constant, and [A]0 is the initial concentration of reactant A. This equation is of the type y=mx+b. Therefore, the plot of 1[A]t versus time is always a straight line with a slope k and a y intercept 1[A]0.

Consider the second-order reaction: 2HI(g)H2(g)+I2(g) Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. What will be the concentration of HI after t = 4.15×1010 s ([HI]t) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures.

Explanation / Answer

Assume

initial concentration to be

Ca0

so..

from the second order reaction:

1/Ca = 1/Ca0 + kt

the slope = k, it is not given

so the best mathematical formula:

solving for C final

1/Ca = 1/Ca0 + k*(4.15*10^10=

Ca = 1/(1/Ca0 + k*(4.15*10^10))

You will need to substitute k, Ca0 to get a numerical value

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