The formation reaction of hydroiodic acid was studied by Max Bodenstein in 1897. The results found by him are given in the following table where "T" is the temperature in Kelvin and k₁ and k₂ are respectively the rate constants for the forward and reverse reaction, given in cm³/mol.s. k2 T (K) k1 300 2.04 x 10-16 2.24 x 10-19 500 2.14 x 10-4 1.66 x 10-6 700 3.02 x 10¹ 5.50 x 10-1 Determine the order of the reaction: Answer: n=2.

The formation reaction of hydroiodic acid was studied by Max Bodenstein in 1897. The results found by him are given in the following table where "T" is the temperature in Kelvin and k₁ and k₂ are respectively the rate constants for the forward and reverse reaction, given in cm³/mol.s. k2 T (K) k1 300 2.04 x 10-16 2.24 x 10-19 500 2.14 x 10-4 1.66 x 10-6 700 3.02 x 10¹ 5.50 x 10-1 Determine the order of the reaction: Answer: n=2.

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

Some measurements of the initial rate of a certain reaction are given in the table below. N2 H2 initial rate of reaction 2.31M 0.547M 89.0M/s 11.0M 0.547M 424. M/s 2.31 M 1.75М 911. 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 = k |I| x10 k = ?
25. Nitrogen(II) oxide reacts with chlorine according to the equation: 2NO(g) + Cl₂(g) →→→ 2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (mol/L¹) [Cl₂] (mol/L) Rate (mol/L/h) 0.50 1.00 1.00 0.50 0.50 1.00 1.14 O 4.56 9.12 What is the rate equation that describes the rate's dependence on the concentrations of NO and Cl₂? What is the rate constant? What are the orders with respect to each reactant? S N
Consider the initial-rate data at a certain temperature in the table for the reaction described by 2 NO₂(g) + O₂(g) → N₂O5 (g) + O₂(g) Determine the value and units of the rate constant, k. k = X10 TOOLS [NO2], (M) [03]o (M) 0.650 0.800 1.10 0.800 1.76 1.40 Units: Initial rate (M/s) 3.12 x 104 5.28 x 104 14.78 x 104
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University 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-1. What is the value of the rate constant at 750.0 K? k = 1.34 x103 Incorrect
Time, s C3H8], M 0.0 0.26 10.0 0.18 20.0 0.14 30.0 0.10 . 40.0 0.064 .50.0 0.052 M
Some measurements of the initial rate of a certain reaction are given in the table below. [N] 0.815M1.56M N,|H||initial rate of reaction 185. M/s 141.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. 口 rate = 0 ロ || = 1 Explanation Check D2022 McGrny Hl LLC. Al Rights Reserved. Terms of N 回至五
A certain reaction has the following general form: aA → bB At a particular temperature and = 2.40 x 10-2 M, concentration versus time data were collected for this reaction, and a plot of [A]o In[A] versus time resulted in a straight line with a slope value of -4.39 x 10-2 min a Determine the rate law for this reaction. Rate = Determine the integrated rate law for this reaction. In[A] = Determine the value of the rate constant for this reaction. Rate constant = min-1
Some measurements of the initial rate of a certain reaction are given in the table below. [H,] [1] initial rate of reaction 0.178M 2.10M 7.00 x 10°M/s 0.0727M 2.10M 2.86 x 10°M/s 0.178M |3.23M 1.08 × 10*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 = k|| x10 k =
Determine the rate law and calculate the rate constant for this reaction: 2 NO (g) + Br₂(1)→2 NOBr (g) Initial [Br₂]/M Expt. 1 2 3 Initial [NO]/M 0.10 0.20 0.20 0.10 0.10 0.30 Initial rate/M.s-¹ 1.30 x 10-³ 5.20 x 10-³ 1.56 x 10-²
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.85M 0.849 M 59.0 M/s 1.85M 0.188M 2.89 M/s 8.12M 0.849 M 259. 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 = k = k ☐x10 •