so2 mol/L |03] mol/L Initial Rate mol/L.s 0.25 0.40 0.118 0.25 0.20 0.118 0.75 0.20 1.062 Q1 Consider the following reactions SO2 + 03 → SO3 +02. A rate study of this reaction was conducted at 298 K. The data that were obtained are shown in the table (a) What is the order of reactions for S02 (b) What is the order of reactions for 03 (c) Write the rate law (d) Determine the value and units of the rate constant, k

so2 mol/L |03] mol/L Initial Rate mol/L.s 0.25 0.40 0.118 0.25 0.20 0.118 0.75 0.20 1.062 Q1 Consider the following reactions SO2 + 03 → SO3 +02. A rate study of this reaction was conducted at 298 K. The data that were obtained are shown in the table (a) What is the order of reactions for S02 (b) What is the order of reactions for 03 (c) Write the rate law (d) Determine the value and units of the rate constant, k

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

3) The rate constant for the reaction 2 N20(g) → 2N2(g) + O2(g) has been found to vary with temperature according to the following data. Determine the activation energy for the reaction. (Must include best fit graph). e 1°C k /s1 565 728 757 780 1.10 x 10-3 0.380 0.871 1.67
Consider the mechanism. Step 1: Step 2: Overall: A B+C C+D E - equilibrium slow A+DB+E Determine the rate law for the overall reaction, where the overall rate constant is represented as k.
2. At 325°C, N0,(g) reacts with CO(g) to yield NO(g) and CO,(g). The reaction is: NO,(g) + CO(g) I NO(g) + CO,(g) It is observed that the reaction rate does not depend upon the concentration of CO, and t\so the reaction rate law does not involve [CO]. The rate does depend upon [NO,], however, and the following data is obtained. Determine the rate law and the value of the rate constant. Rate ( M sec ') NO,] 1. 1 X 10 -2 0.15 4.5 X 10-2 0.3 1.8 X 10- 4.0 X 10-13 0.6 0.9
Nitrogen dioxide is a highly reactive gas! Determine the rate law and the value of k for the following reaction using the data provided: NO,(g) + O,(g) – NO,(g) + 0,(g) (w) P'ONI [0,1 (M) Initial Rate (M' s) 0.10 0.10 0.25 0.33 0.66 1.42 2.84 7.10 0.66 O Rate = 227 M25SINO,10j5 O Rate = 130 M2 s'[NO,10.J O Rate = 430 M2 s 'INO,ř10.] O Rate = 1380 M2.5 5INO, 10,1 O Rate = 43 M SINO,1O,]
3. Consider NO₂ (g) + CO (g) → NO (g) + CO₂ (g). The initial rates are shown in the table below. Please compute (a) the rate law for the reaction and (b) compute the value of k. [CO] 0.050 0.050 0.100 0.100 [NO₂] 0.050 0.100 0.200 0.100 Initial Rate (M/s) 0.0040 0.016 0.256 0.0640
Consider this reaction: 2NH, (g) - N2 (g) +3H, (g) At a certain temperature it obeys this rate law. rate =(0.0103 s")[NH,] S Suppose a vessel contains NH, at a concentration of 0.170M. Calculate the concentration of NH, in the vessel 68.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10
3. The following mechanism is proposed for the reaction of chlorine with chloroform: Cl, + CHCI, CCI, + HCI Cl, Step 1 fast equilibrium 2Cl CHCI, +CI » HCI +CCI, CCI, +Cl»cCI, Step 2 slow Step 3 fast a) Show that this mechanism gives the correct, overall balanced reaction equation. b) Write the rate law predicted by this mechanism.
The rate constant for this zero-order reaction is 0.0240 M •s= at 300 °C. A products > How long (in seconds) would it take for the concentration of A to decrease from 0.890 M to 0.270 M? t = S