For a second-order reaction, [A]âproducts, 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]tversus time is always a straight line with a slope k and a y intercept 1[A]0.
Consider the second-order reaction:
2HI(g)âH2(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 = 2.95Ã1010 s ([HI]t) for a reaction starting under the condition in the simulation?
Express your answer in moles per liters to three significant figures.
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]âproducts, 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 Aat 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]tversus time is always a straight line with a slope k and a y intercept 1[A]0.
Consider the second-order reaction: 2HI(g)âH2(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 = 7.05Ã1010 s ([HI]t) for a reaction starting under the condition in the simulation?
