5. If for the reaction aX +bY Products, the rate law is determined to be r k [X'[Y[', thena. the order of the reaction is 0b. increasing the concentration of Y will have no effect on the ratec. increasing the concentration of X will have no effect on the rated. increasing the concentration ofY will increase the rate of the reactionc. there is no way to determine the value of k

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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...

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8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time
6b please!
Please help me.
Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. so,Cı, (g) → so, (g) + Cl, (g) Rate X' X, +, log, Cos, 12 Part 2 X Feedback O See Hint Remember to use square brackets to show concentration. Do not include multiplication symbols in the rate equation. Do not place spaces in your answer. Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. NO,(2) +Co(g) NO(g) +CO,(e)
O KINETICS AND EQUILIBRIUM = 3/5 Using first- and second-order integrated rate laws Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (1.3 M¹-s¯¹) [₂0₁] olo Suppose a vessel contains N₂O5 at a concentration of 1.20M. Calculate the concentration of N₂O5 in the vessel 7.30 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M X Explanation Check Chelsea V @ EH
1. Determine the equation for solving the average rate of this reaction 2 N2 Os → 4 NO2+ O2 a. In terms of NO2 formation b. In terms of N2Os decomposition 2. Determine the order for the individual reactants in the following reaction, as well as the overall order of reaction: C2H4 + H2 > C2H6 Note: By experimentation, it was found out that the reaction obeys the following rate law: rate=k [C2H4] [H2]? 3. The reaction 4 OH + H2S → SO2+ 2 H2O + Hz is first order with respect to OH and first order with respect to H2S. a. What is the overall reaction order? b. What is the rate equation for the reaction?
L15.
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 2.37M 1.28 M 74.0 M/s 5.43 M 1.28M 2.37M 0.289 M Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit rate = k 388. M/s 16.7 M/s k = x10 ☐☐ X 00 0⁰ S
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 2.04M 1.85 M 27.0M/s 4.07 M 1.85 M 2.04M 2.28 M Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k 107. M/s 41.0 M/s k = 0 □ x10 X 5
I rate Method: Explain how to get the rate law trom calculate the orders (step by step) and the value of k including units caction of A +B C D А. М 20 10 10 B, M 15 45 Rate, M/s 4.88 х 10- 7.37 x 10 2.45 x 10 Run 2 .15
[P4], mol/L [Hz], mol/L Initial Rate, mol/(L s) 0.0110 0.0075 3.20 x 104 0.0110 0.0150 6.40 x 104 0.0220 0.0150 6.39 x 104 A. What is the order with respect to each reactant and the overall reaction order? B. What is the rate law for this reaction? C. Calculate the rate constant, K
The rate of a certain reaction is given by the following rate law: rate =k| N,| H2 -k[N;][H+]° Use this information to answer the questions below. What is the reaction order in N,? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of reaction is 0.620 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 24.0 M / s when [N2] = 1.5 M and [H2] = 0.16 M. Calculate the value of the k = |M -2 -1 •S rate constant. Round your answer to 2 significant digits.

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