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→products
The plot of [A] versus t is linear for the zero-order reaction, the plot of ln[A] versus t is linear for the first-order reaction, and the plot of 1[A] versus t is linear for the second-order reaction. [A] represents the concentration of the reactant A.
Reaction order | Linear plot |
zero | [A] vs. t |
first | ln[A] vs. t |
second | 1[A] vs. t |
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, 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.
Part B
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 = 6.82×1010 s ([HI]t) for a reaction starting under the condition in the simulation?
Express your answer in moles per liters to three significant figures.
Most of the time, the rate of a reaction depends on the concentration of the reactant....
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The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y=mx+by=mx+b. Order Integrated Rate Law Graph Slope 0 [A]=−kt+[A]0[A]=−kt+[A]0 [A] vs. t[A] vs. t −k−k 1 ln[A]=−kt+ln[A]0ln[A]=−kt+ln[A]0 ln[A] vs. tln[A] vs. t −k−k 2 1[A]= kt+1[A]01[A]= kt+1[A]0 1[A] vs. t1[A] vs. t kk A.) The reactant concentration in a zero-order reaction was 0.100 MM after 165 ss and 4.00×10−2 MM after 305 ss . What is the...
± Using Integrated Rate Laws Part A The reactant concentration in a zero-order reaction The integrated rate laws for zero-, first-, and second order reaction may be arranged such that they resemble the equation for a straight line y=mx + b was 9.00x102 M after 155 s and 3.50x102 M after 320 s. What is the rate constant for this reaction? Express your answer with the appropriate units Indicate the multiplication of units, as necessary explicitly either with a multiplication...
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 = 5.92×1010 s ([HI]t) for a reaction starting under the condition in the simulation?
Help please CHEM 122 rate laws Tean Number: Names: versus time, Integrated Dr. Sushilla Knottenbelt): Concentration following table: for the general reaction A orders. products for the different reaction Linear form-what should Half life equation be graphed, y vs x to get a straight line? What will the slope (m) be? The y-axis intercept? Reaction Rate form order integrated form Linear form-what Rate = k 2K x=t m--k I Rote In 2 k tın 2 Rate k[A m-K 2. The...
The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y=mx+by=mx+b. Order Integrated Rate Law Graph Slope 0 [A]=−kt+[A]0[A]=−kt+[A]0 [A] vs. t[A] vs. t −k 1 ln[A]=−kt+ln[A]0ln[A]=−kt+ln[A]0 ln[A] vs. tln[A] vs. t −k 2 1[A]= kt+1[A]01[A]= kt+1[A]0 1[A] vs. t1[A] vs. t k Part A The reactant concentration in a zero-order reaction was 8.00×10−2 MM after 130 ss and 4.00×10−2 MM after 380 ss . What is...
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