Please fast solve how do i findthe rate?[MnOs ]o0.00100.00200.00 100.0010Rate [MnOs']o/t[HCIJ.O. luOlu0.160.32Trial0.100.10O. 20C. 1014.forgot this part16 H+ 2 Mn0, + 10 → 5 2 + 2 Mn?+ + 8 H;0TrialmL 0.0050mL 0.50 Mr mL 0.80 Mml H;0Time, sM MnOHCI110101020200201010101043102010109741010201049

how do i find the rate? [MnOs]o 0.0010 0.0020 0.00 10 0.00 to Trial Rate [MnOs]Jo/t O.10 0.10 0.10 O. 10 (HC]Jo O. lu Olu 0.16 0.32 1 2 3 4. forgot this part 16 H+2 Mno, + 10 → 5 a + 2 Mn? + 8 H;0 Trial mL 0.0050 ml 0.50 MI ml 0.80 M mL H20 Time, s M MnO HCI 10 10 10 20 200 20 10 10 10 104 3 10 20 10 10 97 4. 10 10 20 10 49

how do i find the rate? [MnOs]o 0.0010 0.0020 0.00 10 0.00 to Trial Rate [MnOs]Jo/t O.10 0.10 0.10 O. 10 (HC]Jo O. lu Olu 0.16 0.32 1 2 3 4. forgot this part 16 H+2 Mno, + 10 → 5 a + 2 Mn? + 8 H;0 Trial mL 0.0050 ml 0.50 MI ml 0.80 M mL H20 Time, s M MnO HCI 10 10 10 20 200 20 10 10 10 104 3 10 20 10 10 97 4. 10 10 20 10 49

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter16: Reaction Rates

Section: Chapter Questions

Problem 6STP

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The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103
Consider the following hypothetical reaction: 2AB2(g)A2(g)+2B2(g)A 500.0-mL flask is filled with 0.384 mol of AB2. The appearance of A2 is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. (a) Make a similar table for the disappearance of AB2. (b) What is the average rate of disappearance of AB2 over the second and third 10-minute intervals? (c) What is the average rate of appearance of A2 between t=30 and t=50?