Learning Goal:To understand zero-order reactions.Chemical kinetics is the study of the speed with which a chemical reaction occurs and thefactors that affect this speed. The speed of a reaction is the rate at which theconcentrations of reactants and products change. This relationship is expressed throughrate laws.For a general reaction aA + bBgG+ hH, the rate law is given asrate of reaction= k[A] [B]"where the coefficients and are experimentally determined while a, b, g, and h arestoichiometric coefficients unrelated to me and nAzero-order reaction has a rate law in which the sum of the exponents m +n + ... isequal to zero. Thus, if there is only one reactant, the rate of reaction is independent of theconcentration of the reactant.For a zero-order reaction, the graph of reactant concentration versus time is a straight line.Therefore, the rate-law equation for a zero-order reaction can be compared to that of astraight line, y = mz+b✓ CorrectImportant: If you use this answer in later parts, use the full unrounded value in your calculations.The faster the reaction, the shorter the half-life for that reaction. The rate of the reaction is proportional to rate constant; thus, the larger the rate constant, the shorter the half-life.Part DIn a certain hypothetical experiment, the initial concentration of the reactant R is 1.00 mol-L, and its rate constant is 0.0150 mol-Ls. It follows a zero-order reaction mechanism for the consumption ofreactant R. Plot the graph of concentration versus time. Consider the time intervals as 0, 10, 20, 30, 40, and 50 s.Then select the appropriate graph and plot the appropriate points.▸ View Available Hint(s)No elements selectedSubmit20.9024055 60Select the elements from the list and add them to the canvas setting the appropriate attributes. Press (TAB) to get to themain menu.

To plot the graph, we would use the integrated rate law equation of zero order reaction to calculate…

In a certain hypothetical experiment, the initial concentration of the reactant Ris 1.00 mol-Land its rate constant is 0.0150 mol-Ls. It follows a zero-order reaction mechanism for the consumption of reactant R. Plot the graph of concentration versus time. Consider the time intervals as 0, 10, 20, 30, 40, and 50 s Then select the appropriate graph and plot the appropriate points. ▸ View Available Hint(s) No elements selected bil "" 05 04- 03 + 02 20 25 30 45 Select the elements from the list and add them to the canvas setting the appropriate attributes. Press (TB) to get to the main menu.

In a certain hypothetical experiment, the initial concentration of the reactant Ris 1.00 mol-Land its rate constant is 0.0150 mol-Ls. It follows a zero-order reaction mechanism for the consumption of reactant R. Plot the graph of concentration versus time. Consider the time intervals as 0, 10, 20, 30, 40, and 50 s Then select the appropriate graph and plot the appropriate points. ▸ View Available Hint(s) No elements selected bil "" 05 04- 03 + 02 20 25 30 45 Select the elements from the list and add them to the canvas setting the appropriate attributes. Press (TB) to get to the main menu.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 3RQ: One experimental procedure that can be used to determine the rate law of a reaction is the method of...

See similar textbooks

Similar questions

The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
Many biochemical reactions are catalyzed by acids. A typical mechanism consistent with the experimental results (in which HA is the acid and X is the reactant) is Step 1: Step 2: Step 3: Derive the rate law from this mechanism. Determine the order of reaction with respect to HA. Determine how doubling the concentration of HA would affect the rate of the reaction.
If you know some calculus, derive the integrated first-order rate law for the reaction by following these steps: Define the reaction rate in terms of [A]. Write the rate law in terms of [A], k, and t. Separate variables in the rate law. Integrate the rate law. Write the integrated equation in the form . Derive the half-life as was done in Section 11-3c.
You are studying the kinetics of the reaction H2(g) + F2(g) 2HF(g) and you wish to determine a mechanism for the reaction. You run the reaction twice by keeping one reactant at a much higher pressure than the other reactant (this lower-pressure reactant begins at 1.000 atm). Unfortunately, you neglect to record which reactant was at the higher pressure, and you forget which it was later. Your data for the first experiment are: Pressure of HF (atm) Time(min) 0 0 0.300 30.0 0.600 65.8 0.900 110.4 1.200 169.1 1.500 255.9 When you ran the second experiment (in which the higher pressure reactant was run at a much higher pressure), you determine the values of the apparent rate constants to be the same. It also turns out that you find data taken from another person in the lab. This individual found that the reaction proceeds 40.0 times faster at 55C than at 35C. You also know, from the energy-level diagram, that there are three steps to the mechanism, and the first step has the highest activation energy. You look up the bond energies of the species involved and they are (in kJ/mol): H8H (432), F8F (154), and H8F (565). a. Sketch an energy-level diagram (qualitative) that is consistent with the one described previously. Hint: See Exercise 106. b. Develop a reasonable mechanism for the reaction. c. Which reactant was limiting in the experiments?
Isomerization of CH3NC occurs slowly when CH3NC is heated. CH3NC(g) CH3CN(g) To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph. (a) What is the rate law for this reaction? (b) What is the equation for the straight line in this graph? (c) Calculate the rate constant for this reaction. (d) How long does it take for half of the sample to isomerize? (e) What is the concentration of CH3NC after 1.0 104 s?
Nitryl fluoride is an explosive compound that can be made by oxidizing nitrogen dioxide with fluorine: 2 NO2(g) + F2(g) → 2 NO2F(g) Several kinetics experiments, all done at the same temperature and involving formation of nitryl fluoride, are summarized in this table: Write the rate law for the reaction. Determine what the order of the reaction is with respect to each reactant and each product. Calculate the rate constant k and express it in appropriate units.
At 500 K in the presence of a copper surface, ethanol decomposes according to the equation C2H5OH(g)CH3CHO(g)+H2(g) The pressure of C2H5OH was measured as a function of time and the following data were obtained: Time(s) PC2H5OH(torr) 0 250. 100. 237 200. 224 300. 211 400. 198 500. 185 Since the pressure of a gas is directly proportional to the concentration of gas, we can express the rate law for a gaseous reaction in terms of partial pressures. Using the above data, deduce the rate law, the integrated rate law, and the value of the rate constant, all in terms of pressure units in atm and time in seconds. Predict the pressure of C2H5OH after 900. s from the start of the reaction. (Hint: To determine the order of the reaction with respect to C2H5OH, compare how the pressure of C2H5OH decreases with each time listing.)
When enzymes are present at very low concentration, their effect on reaction rate can be described by first-order kinetics. Calculate by what factor the rate of an enzyme-catalyzed reaction changes when the enzyme concentration is changed from 1.5 107 M to 4.5 106 M.