Consider the following reaction: RX;Y+ 3Y2 → RY++ 3XY. A series of reactions were carried out at 100°C to yield the databelow.Trial Initial molarity, RX:Y Initial molarity, YıInitial rate (M/sec)10.850.250.5622.550.250.56a. Based on the data, what is the order with respect to RX; Y?b. If the order with respect to Yı is second order, calculate the rate constant for the reaction.

The rate of reaction depends on the concentration of the reactants that participating in the slowest…

Consider the following reaction: RX)Y + 3Y; - RY«+ 3XY. A series of reactions were carried out at 100°C to yield the data below. Trial initial molarity, RX)Y Initial molarity, Y: Initial rate (M/sec) 0.25 0.25 0.85 2.55 0.56 0.56 a. Based on the data, what is the order with respect to RX Y? b. If the order with respect to Y: is second order, calculate the rate constant for the reaction.

Consider the following reaction: RX)Y + 3Y; - RY«+ 3XY. A series of reactions were carried out at 100°C to yield the data below. Trial initial molarity, RX)Y Initial molarity, Y: Initial rate (M/sec) 0.25 0.25 0.85 2.55 0.56 0.56 a. Based on the data, what is the order with respect to RX Y? b. If the order with respect to Y: is second order, calculate the rate constant for the reaction.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For the following questions (c and d), assume that the concentration of the hydroxide ion was initially 1.00 M, 3.00 M and 5.00 M (after mixing) for Runs #1, #2 and #3, respectively. c. Produce a plot of the pseudo-rate constants, Ln(k') vs. Ln[OH-], Calculation #7 on pg. 7. Determine the order of the hydroxide ion (Attach the relevant spreadsheet and plot). Order of OH-:__ (express as an integer) d. Using the intercept from the plot produced in 2c, determine the value for the rate constant, as described in Calculation #8 on pg. 7 k: 0.2647 Show your work here: K = e-3.6317 = 0.2647 3. Using the analysis in Question #2, determine the rate of reaction of chloromethane with the hydroxide ion at 61 °C, given initial concentrations of [CH3Cl] = [OH-] = 0.45 M?
Expt. 1 2 3 NH; (aq) + NO; (aq) >Nz (aq) + 2 H2O (l) [NO₂] Rate (at 298 K) 0.020 M/s 0.020 M 0.020 M 0.030 M/s 0.010 M 0.0050 M/s [NH+] 0.010 M 0.015 M 0.010 M Determine the complete rate law (rate law and rate constant) for the reaction. Show all work. What is the initial rate of this reaction if the concentrations in Expt. 2 above are tripled. Show work. What is the rate of H₂O formation in Expt. 1? A 4th trial is conducted at 273 K, using the concentrations from Expt. 1. If the rate was found to be 0.016 M/s, calculate the activation energy of this reaction.
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.91×10-4 Ms and a y-intercept of 0.235 M. Based on this plot, the reaction is reaction is order in HI and the rate constant for the Ms!
Part II. Solve each of the following problems. A. Iodide ion is oxidized to hypoiodite ion, IO", by hypochlorite ion, CIOʻin basic solution. The equation is I (aq) + Cl0" (aq) + OH° → I0' (aq) + Cl (aq) + H20 The following data were obtained for initial rates Expt. [I] (M) [CIO'] (M) [ОН] (М) Rate (mol/L s) 12.2 X 10-2 12.2 X 10 -2 6.1 X 10 -2 3.0 X 102 1 0.010 0.020 0.010 2 0.020 0.010 0.010 3 0.010 0.010 0.020 4 0.010 0.010 0.010 Calculate the order of the reaction with respect to I; with respect to CIO; with respect to OH; and the overall order of reaction. What is the rate constant of the reaction? The reaction is done at 22.0 C. It is determined that the activation energy of the reaction is 62 kJ/ mol. What is the rate constant of the reaction at 27.0 C
The reaction 2 H2O2(aq) ➝ 2 H2O(l) + O2(g) is first order in H2O2 and under certain conditions has a rate constant of k = 0.00752 s-1 at 20.0ºC. A reaction vessel initially contains 150.0 mL of 30.0 % H2O2 by mass solution. The density of the solution is 1.11 g/mL. The gaseous oxygen is collected over water at 20.0ºC as it forms. What volume of O2 forms in 85.0 seconds at a barometric pressure of 742.5 mmHg? The vapor pressure of water at this temperature is 17.5 mmHg.
Consider the base hydrolysis of an ester.RCOOR' + OH− → RCOO− + R'OH (where R and R' represent organic groups).The kinetics of this reaction, for a particular ester, were studied using the isolation method. When [OH−] << [RCOOR'] a pseudo-rate law can be posed:-d[OH-] / dt = k'' [OH-]mWith initial concentrations: [OH−]0 = 0.0015 M [RCOOR']0 = 0.700 M a plot of ln[OH-] versus t gave a straight line with slope = -0.0176 s-1 and y-intercept = -6.50.What is the order "m"?m = ? What is the corresponding pseudo rate constant k''? (include appropriate units)k'' = ?
The following mechanism for the gas phase decomposition of oxygen difluoride is consistent with the observed rate law. step 1 fast: 2 OF2=0;F4 step 2 slow: 0,F4¬0; +2 F; (1) What is the cquation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"|B]". , where 'I' is understood (so don't write it if it's a 'l') for m, n etc.
(2) The reaction-rate data given below were obtained using a batch reaction system for the reaction A→products. Plot the data in appropriate form to test the fit for zero- and first-order kinetics. From the plot that gives the best fit, determine the appropriate reaction rate constant (remember the units). Time, min CA, (g/m3) 0 30 0.5 25.4 1 21.6 2 16.9 4 13.1 8 8.3 16 3.2 32 0.31
Please explain how to find rate constant (k) if reaction rate = 3.40*10^-7 I^- molar = .00200 (reaction order 1) BrO3^- molar = .00800 (reaction order 1) H^+ molar = .0400 (reaction order 2)
The overall gas phase reaction 3A --> B + 2C occurs via the following sequence of elementary steps 2A <--> I1 + B k1,k2 A + I1 --> 2I2 k2 I2 --> C k3 1. write an expression for the overall reaction rate, r, in terms of the rate step 3, r3 2. using the answer from 1, obtain an expression for the reaction rate, r, in terms of rate constants and concentrations of reactants and products, only use PSSH. 3. State the. specific inequality the must be satisfied for each of the following assumptions to hold, and use it to simplify the general rate expression from question 2. i) Step 1 is quasi-equilibrium ii) Step 1 is irreversible
Why does the product (a•b), rather than the sum (a + b) appear in the Law of Mass Action? This is sometimes brought up to demonstrate how/why nonlinear terms arise in differential equations. The law of mass action states that The rate of a chemical reaction involving an interaction of two or more chemical species is proportional to the product of the concentrations of the given species. This is NOT an assignment...I'm just curious and trying to understand mathematical relations better. Thanks!
Chlorine dioxide, Cl02, is a reddish-yellow gas that is soluble in water. In basic solution it gives Cl03- and CIO2 ions. 2C1O:(aq) + 20н (ад) —> СIО3 (aд) + CIO, (aq) + H;0(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Initial Concentration Initial Concentration Initial Rate of Cl02 (mol/L) of OH (mol/L) (mol(L's) Exp. 1 0.21 1.6 x 10-2 0.162 Exp. 2 7.0 x 10-2 1.6 x 10-2 1.80 x 10-2 Exp. 3 7.0 x 10-2 4.8 x 10-2 5.39 х 10-2 a Obtain the rate law. (Use k for the rate constant.) Rate law =