L山 Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2 initial rate of reaction 0.708M 2.02M 71.0M/s 2.29M 2.02M 743.M/s 0.708M 0.571M 20.1M/s 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 3 significant digits. Also be sure your answer has the correct unit symbol. %3D Check Save For Later O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use P. EPIC ... MacBook Pro 888 F4 F3 F5 F10 $ # 3 5. 6. R. ock C B. W. alt option command commar

L山 Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2 initial rate of reaction 0.708M 2.02M 71.0M/s 2.29M 2.02M 743.M/s 0.708M 0.571M 20.1M/s 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 3 significant digits. Also be sure your answer has the correct unit symbol. %3D Check Save For Later O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use P. EPIC ... MacBook Pro 888 F4 F3 F5 F10 $ # 3 5. 6. R. ock C B. W. alt option command commar

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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Some measurements of the initial rate of a certain reaction are given in the table below. N₂ [H₂] initial rate of reaction 1.85M 0.232M 1.85M 0.899M 6.27M 0.232M rate=& 3.00M/s 45.0M/s 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. k = 0 34.5 M/s G x10 ロ・ロ X 00
For the reaction: 4NH3 (g) + 7O2 (g) → 4NO2 (g) + 6H2 (g), if H2 is produced at a rate of 3.5 x 10-3 M/s, O2 is consumed at a rate of... A. -2.5 x 10-2 M/s B. -4.1 x 10-3 M/s C. -2.1 x 10-2 M/s D. -3.0 x 10-3 M/s E. -5.8 x 10-4 M/s
6. For the reaction CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(1), what can be said about the order(s) of reaction for this rate law? a. The order is 1. b. The orders are 1 and 2 for CH4 and O2, respectively. c. The order cannot be determined when the reaction involves different phases of matter. d. The order must be determined experimentally.
Some measurements of the initial rate of a certain reaction are given in the table below. [H₂] [12] initial rate of reaction 2.12M 1.97M 0.366 M/s 2.12M 0.560 M 0.104 M/s 0.408 M 1.97M 0.0704 M/s 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 k = Continue 0 x10 ロ・ロ © 2023 McGraw Hill LLC. All Rights Reser
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 0.285M 1.73M 87.0 M/s 0.285M 7.20 M 1.51 × 10³ M/s 1.19M 1.73M 1.52 × 10³ M/s 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 3 significant digits. Also be sure your answer has the correct unit symbol. rate = & 0 0.0 k = 0 X ?
5. The following initial rate data were obtained for the reaction a. C. 2C1O₂(aq) + 2OH(aq) → CIO3(aq) + ClO₂ + H₂O [CIO₂] 0.024 0.018 0.024 Write the rate law for this reaction. [OH-] 0.011 0.011 0.014 b. Calculate the rate constant and specify units. Initial Rate (Mos¹) 7.27 x 10-4 4.09 x 10-4 9.25 x 10-4 Calculate the rate when the [CIO₂] = 0.75 M and [OH-] = 0.0250 M.
The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 9.90 × 10-10 cm³ molecule-¹.s-¹ at 298 K. Convert the rate constant to units of M-¹.s-¹. k = k = Incorrect Convert the rate constant to units of Torr-¹.s-¹. 5.962 ×10¹7 Incorrect 2 3.208 ×10¹7 What is the order of this reaction? 0 M-¹.s Torr-g
Refer to the following reaction: NO2(g) + CO(g) → NO(g) + CO2(g). If the reaction is second order with respect to both NO2 and CO, what happens to the reaction rate when the concentration of both reactants is doubled? O Reaction rate is also doubled O Reaction rate increases by a factor of 8 O Reaction rate increases by a factor of 16 Reaction rate increases by a factor of 32
Consider the following reaction: 2N₂O(g) → 2N2(g) + O2(g) Part A Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. Rate = 1 A[₂0] At O Rate = O Rate - Submit Rate = -A[₂0] At Correct Part B Rate = Submit A[N₂O] At Part C A[N₂0] At A[N₂O] At Previous Answers Submit Request Answer 1 A[N₂] 2 At At In the first 13.0 s of the reaction, 1.9x10-2 mol of O₂ is produced in a reaction vessel with a volume of 0.280 L. What is the average rate of the reaction over this time interval? Express your answer using two significant figures. IVE| ΑΣΦ Request Answer A[N₂] At 1 A[N₂] At 1/1 A[0₂] At A[0₂] At A[0₂] A[0₂] At Predict the rate of change in the concentration of N₂O over this time interval. In other words, what is A[N₂O]/At? Express your answer using two significant figures. IVE| ΑΣΦ ? M-s-1 ? M-s-1
Describe one example in real life of a factor affecting the rate of a specific reaction.
For the reaction 2 X --- Y + Z, the rate constant is 0.0543 L.mol-1s-1 at 23 oC. The rate constant increases to 0.1086 L.mol-1s-1 at 33 oC. What is the frequency factor for the reaction? A. 1.78 x 108 B. 9.30 x 107 C. 7.85 x 108 D. 8.80 x 107 E. 6.84 x 109
Consider the following gas-phase reaction. A(g) + 2B(g) → C(g) Use the data set to determine the order of the reaction in A, the order in B, the overall order and the rate law, including the value of the rate constant. Initial concentration A (mol L-1) Initial concentration B (mol L-1) Initial Rate (mol L-1 s-1) 0.12 0.32 3.60 x 10-4 0.12 0.64 3.60 x 10-4 0.24 0.32 7.20 x 10-4 Use the rate law that you have found to determine the initial rate of the reaction if the initial concentrations are [A] = 0.33 mol L-1 and [B] = 0.46 mol L-1. How is the rate of appearance of C related to the rate of disappearance of B?