The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseousreaction 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 =5.55 ×10¹1IncorrectConvert the rate constant to units of Torr-¹.s-¹.-11.84 ×10⁹Incorrect2013What is the order of this reaction?M-¹.s-1Torr-¹.s-1

The rate constant gives the relationship between the molar concentration of the reactant and the…

The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 9.90 x 10-10 cm³ molecule-¹.s at 298 K. Convert the rate constant to units of M-¹.s-¹. k = k= 5.55 ×10¹1 Incorrect Convert the rate constant to units of Torr-¹.s-¹. 1.84 ×10⁹ Incorrect 2 0 1 3 What is the order of this reaction? M-1.s-1 Torr-1.s-1

The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 9.90 x 10-10 cm³ molecule-¹.s at 298 K. Convert the rate constant to units of M-¹.s-¹. k = k= 5.55 ×10¹1 Incorrect Convert the rate constant to units of Torr-¹.s-¹. 1.84 ×10⁹ Incorrect 2 0 1 3 What is the order of this reaction? M-1.s-1 Torr-1.s-1

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

General Chemistry 4th Edition McQuarrie • Rock • Gallogly dUniversity Science Books presented by Macmillan Learning The reaction C,H¿ (g) → 2 C,H¿(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-!. What is the value of the rate constant at 840.0 K? k =
4. Given: A +B O C Rate ( M sec ') 4.0X 10 -5 4.0 X 105 16 X 10-5 [] 0.1 [B] 0.1 0.1 0.2 0.2 0.1 Determine the rate law. Calculate the rate constant. Determine the rate when [A] = 0.05 and [B] = 0.10
D
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. 1 rate = (0.471 M¹S -¹) [N₂05]² Suppose a vessel contains N₂O5 at a concentration of 0.800M. Calculate the concentration of N₂O5 in the vessel 8.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10
The following data was collected for the reaction 2 Mg + O2 --> 2MgO Determine the order for each reactant and write the rate law. Trial [Mg] (mol/L) [O2] (mol/L) Measured Rate(M/s) 1 .10 .10 2.0x10-3 2 .20 .10 4.0x10-3 3 .10 .20 8.0x10-3 According to this data the order for Mg is Answer (enter a number).
Ⓒ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Data
A certain reaction has the following rate law: rate = k[X]³[Y]² Which of the following are the correct units for k? Select one: L³mol-3s-1 Ms-1 M³s O L?mol2s1 L5mol 5s1 Lmol-'s mol³L-3s-1 M's-1 L*mol-4s-1 mol?L-2s1
What is the rate law for this reaction? Br Na CH;S S SCH3 DMSO ORate = k [C6H11 ] CH, Br ORate k [C6H11 CH2 SCH3] [CH3 S] ORate k [CH3 S ] O Rate k [C6H11 ] [CH3 S] CH, Br
Q6
g.
Consider this reaction: 2C1₂0, (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate = (1.31 M¹-8¹)[Chos S Suppose a vessel contains Cl₂O5 at a concentration of 0.690 M. Calculate the concentration of C1₂O5 in the vessel 3.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M ? CU x10 X S