The tabulated data were collected for this reaction at a certain temperature: X 2 Y → 2 X + Y a. Determine the order of the reaction and the value of the rate constant at this temperature.

Identify the general form of the rate law for the reaction, which can be expressed as Rate = k[X 2 Y] n , where k is the rate constant, [X 2 Y] is the concentration of the reactant, and n is the order of the reaction with respect to X 2 Y.. Plot the provided concentration data of X 2 Y against time on a graph to visually inspect how the concentration changes. This can help in determining the reaction order by looking at the shape of the curve.. To determine the order of the reaction (n), try fitting the data to different kinetic models: zero-order (plot [X 2 Y] vs. time), first-order (plot ln([X 2 Y]) vs. time), and second-order (plot 1/[X 2 Y] vs. time). The plot that results in a straight line indicates the order of the reaction.. Once the order of the reaction is determined from the best-fit line, use the slope of this line to calculate the rate constant (k). The relationship between the slope and k depends on the order of the reaction: for zero-order, slope = -k; for first-order, slope = -k; for second-order, slope = k.. Compile the results to summarize the order of the reaction and the value of the rate constant (k) at the given temperature.

The tabulated data were collected for this reaction at a certain temperature: X 2 Y → 2 X + Y a. Determine the order of the reaction and the value of the rate constant at this temperature.

Hello. In this problem we are told for the reaction A. Goes to form be the concentration of a. Is observed over time and tabulated and reported in the table below, we are asked to determine the rate order and calculate the reaction rate constant. In order to do this, we're going to need to make use of the integrated rate laws. Beginning with then Reactions of Order zero. The integrated rate law is given by the concentration of A. At time. T. Is equal to the negative of a reaction rate constant times time plus our initial concentration of A. If we have a zero order reaction and we make a plot of concentration of A versus T. And it's a straight line, the slope will be equal to minus K. And the reason is that this integrated rate law takes the form of a straight line. And so all integrated rate laws take the form of a straight line in case of a first order reaction. If we make a plot of the natural log of A versus time we'll get a straight line and the slope will be equal to the negative of a reaction rate constant. If we have a second order reaction again, the integrated rate law will take the form of a straight line. If we plot one over the concentration of A versus time, we'll get then a straight line with our slope equal to the reaction rate constant. So what we need to do then is take our data and we need to calculate the natural log of concentration of A. And we need to find one over the concentration of A. And then generate three plots within are going to look at which plot as the best fit line. If we make these three plots in a program like Excel, we'll find then the plot of one over the concentration versus time produces a straight line. So this is the best fit line with an R. Squared value of one. And we see then that the slope of the line is equal to 0.0446. So this is then equal to our reaction rate constant. If we then consider our units keep in mind that we're finding the slope of the line, which is the change in Y. Over the change in X. So our units then why are one over more clarity and then change in X. Which is our time is second. So our concentrations work out to per polarity per second. And this is then again a plot for a second order reaction. And so we find our reaction rate constant for the second order reaction is 0.0446 per Moleketi per second. Thanks for watching. Hope this helps

Ch.14 - Chemical Kinetics

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Tro 4th Edition

Ch.14 - Chemical Kinetics

Problem 84a

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Chapter 14, Problem 84a

The tabulated data were collected for this reaction at a certain temperature: X₂Y → 2 X + Y a. Determine the order of the reaction and the value of the rate constant at this temperature.

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Identify the general form of the rate law for the reaction, which can be expressed as Rate = k[X2Y]n, where k is the rate constant, [X2Y] is the concentration of the reactant, and n is the order of the reaction with respect to X2Y.

Plot the provided concentration data of X2Y against time on a graph to visually inspect how the concentration changes. This can help in determining the reaction order by looking at the shape of the curve.

To determine the order of the reaction (n), try fitting the data to different kinetic models: zero-order (plot [X2Y] vs. time), first-order (plot ln([X2Y]) vs. time), and second-order (plot 1/[X2Y] vs. time). The plot that results in a straight line indicates the order of the reaction.

Once the order of the reaction is determined from the best-fit line, use the slope of this line to calculate the rate constant (k). The relationship between the slope and k depends on the order of the reaction: for zero-order, slope = -k; for first-order, slope = -k; for second-order, slope = k.

Compile the results to summarize the order of the reaction and the value of the rate constant (k) at the given temperature.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Reaction Order

The order of a reaction refers to the power to which the concentration of a reactant is raised in the rate law. It indicates how the rate of reaction depends on the concentration of reactants. For example, a first-order reaction depends linearly on the concentration of one reactant, while a second-order reaction depends on the square of the concentration. Understanding the reaction order is crucial for determining how changes in concentration affect the reaction rate.

Rate Law

The rate law is an equation that relates the rate of a chemical reaction to the concentration of its reactants. It is typically expressed in the form Rate = k[A]^m[B]^n, where k is the rate constant, and m and n are the orders of the reaction with respect to reactants A and B, respectively. The rate law is determined experimentally and is essential for calculating the rate constant and understanding the kinetics of the reaction.

Rate Constant (k)

The rate constant, denoted as k, is a proportionality factor in the rate law that is specific to a particular reaction at a given temperature. It reflects the speed of the reaction; a larger k indicates a faster reaction. The value of k can be determined from experimental data and is influenced by factors such as temperature and the presence of catalysts. Understanding k is vital for predicting how quickly a reaction will proceed under specific conditions.