SEAT WORK # 3: 1.) THE RATE OF THE REACTION BETWEEN CO AND NO₂ CO(g) + NO₂ (a) → CO₂ (g) + No (a). WAS STUDIED AT 540 K WITH VARIOUS CONCENTRATIONS OF CO AND NO₂, AWD THE DATA IN THE TABLE WERE COLLECTED DETERMINE THE RATE EQUATION AND THE VALUE OF THE RATE CONSTANT. 400 br nuppupS VIL DUR!

SEAT WORK # 3: 1.) THE RATE OF THE REACTION BETWEEN CO AND NO₂ CO(g) + NO₂ (a) → CO₂ (g) + No (a). WAS STUDIED AT 540 K WITH VARIOUS CONCENTRATIONS OF CO AND NO₂, AWD THE DATA IN THE TABLE WERE COLLECTED DETERMINE THE RATE EQUATION AND THE VALUE OF THE RATE CONSTANT. 400 br nuppupS VIL DUR!

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

2. Consider the reaction that occurs when a CIO2 solution and a solution containing hydroxide ions (OH) are mixed at 0°C, shown in the following equation. 2CIO2(aq) + 2OH (aq) → Cl03° (aq) + CIO2° (aq) + H2O (1) When solutions containing CIO2 and OH- in various concentrations were mixed at 0 oC, the following rate data were obtained: Determination Initial concentration Initial concentration of Initial rate for formation number of ClO2, mol/L OH", mol/L of CIO3¯ mol/Ls 1.25x10-2 1.30x10-3 2.33x10-4 2.50x10-2 1.30x10-3 9.34x104 3 2.50x10-2 2.60x103 1.87x10-3 a) Use the method of initial rates to find the order of the reaction with respect to CIO2 and with respect to OH. Write the rate equation for the reaction of CIO2 and OH´ at 0°C. b) Calculate the rate constant, k, for the reaction of clO2 and OH at 0°C. c) Calculate the reaction rate for the reaction CIO2 and OH at 0°C when the initial ClO2 and OH concentrations are 8.25x10-3 mol/L and 5.35x 10-² mol/L, respectively. 1.
Correct Expressed in terms of x, y, and z, the rate law is as follows: The iodate ion, IO3¯, is reduced by sulfite, SO32", according to the following net ionic equation: rate = kæyz By substituting the actual species from the reaction, the expression becomes I03 (aq) + 3S03²- (aq)→I¯(aq) + 3SO,²-(aq) k[IO3 ][SO3²-][H*] rate = Part B By what factor will the rate of the reaction change if the pH changes from 6.50 to 2.00? Express your answer numerically using two significant figures. • View Available Hint(s) 3.2 • 10-5 Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Because it is less than one, your answer implies that the rate decreases. However, lowering the pH raises the hydrogen ion concentration. Part C The reaction is pH dependent even though the H+ ion does not appear in the overall reaction. Which of the following explains this observation? Check all that apply. • View Available Hint(s) O H+ serves as a catalyst in the reaction. The exponent of H+ in the rate…
Consider the following reaction: 5Br (ag) + BrO;¯(aq) + 6H*(aq) → 3Br,(aq) + 3H,O() If the rate of disappearance of Br(ag) at a particular moment during the reaction is 3.5×10 mol L-1s-1, what is the rate of disappearance of BrO (aq) at that moment? O 5.8x 10 mol Ls? 07.0x 10 mol Ls! 0 3.5x 10 mol Lis
See image below. Can you please show me how to solve this problem?
Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0013 M ·s : 2N,0 (g) → 2N, (g) +0, (3) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of dinitrogen monoxide. After how much time is there only 200. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 믐
Consider this reaction: NH,OH (aq) → NH, (aq) +H,0(aq) At a certain temperature it obeys this rate law. [NH, OH] rate = (1.32 M -1 •S Suppose a vessel contains NH¸OH at a concentration of 0.710 M. Calculate how long it takes for the concentration of NH¸OH to decrease by 83.0%. You may assume no other reaction is important.
1) Please help
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
Last part of this question... An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 → 2NH3. Starting with a closed reactor containing 1.25 mol/L of N2 and 0.35 mol/L of H2, she finds that the H2 concentration has fallen to 0.12 mol/L after 40. seconds. What is the average rate of reaction of H2 over this time? (Enter in mol/liter/sec). 0.0058 You are correct.Your receipt no. is 155-176 Previous Tries What is the average rate of NH3 production for this example? (Enter in mol/liter/sec). 0.0038 You are correct.Your receipt no. is 155-8777 Previous Tries Estimate the N2 concentration after 40 seconds? (Enter in mol/liter).
Q3
A reaction proceeds according to the following equation: A + 3B → 2C + 2D At an early stage of the reaction, conc. A = 1.991 M and 5.23 minutes later, conc. A= 0.861 M. What is the average rate of the reaction during this time period, expressed in units of M·s-1? Report your answer with four decimals. Enter numbers only; do not enter units.
I completed the problem but for some reason, my answer is still wrong. for part a I got 5.48 x 10^-5 and for part b I got 5.61x10^-4. I substituted the concentrations in the equation but hey still seem to be wrong can someone explain?