The reaction AB(aq) -has a rate constant of 0.0118 M-1.s-'at 25.0°C. A reaction ves-A(g) + B(g) is second order in AB andsel initially contains 250.0 mL of 0.100 M AB that is allowed toreact to form the gaseous product. The product is collected overwater at 25.0 °C. How much time is required to produce 200.0ml. of the products at a barometric pressure of 755.1 mmHg?(The vapor pressure of water at this temperature is 23.8 mmHg.)

The given reaction is second-order hence rate law: Reaction: Data are given: The initial…

Answered: The reaction AB(aq) - has a rate…

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

13
The following data are for the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C. H202(aq)- → H20(1) + ½ 02(g) [ H202 ], M 2.18x10-2 1.09x10-2 5.45x10-3 2.73x10-3 time, min 8.40 16.8 25.2 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is min . (2) Based on these data, the rate constant for this O order reaction is min -1.
Arrange the following reactions in order of increasing rate (slowest to fastest) i. CzsHs2 (s) + 38 O2 (8) → 5 CO2 (g) + 26 H20 () ii. Ag* (aq) + I'(aq) > Agl (s) iii. H2 (g) + % O2 (8) → H20 a. i, ii, ii b. iii, ii, i c. ii, i, ii d. ii, i, iii e. ii, ii, i
1. The decomposition of hydrogen peroxide (H2O2) was observed and yielded the results shown below. Time (s) [H2O2] (mol/L) 1.00 120 0.91 300 0.78 600 0.59 1200 0.37 1800 0.22 2400 0.13 3000 0.082 3600 0.050 а. Determine the reaction order of the decomposition of Hydrogen Peroxide b. What is the value of its rate constant?
For the reaction: X + Y --> Z, the reaction rate is found to depend only upon the concentration of X. A plot of 1/X verses time gives a straight line with the equation y=3.35x10-2 X + 0.200 Which of the following is correct. Select one: a. The reaction is second order for X and zero order for Y and k=3.35x10-2 M-1s-1 b. The reaction is second order for both X and Y and k=3.35x10-2 M-1s-1 c. The reaction is zero order for both X and Y and k=3.35x10-2 M-1s-1 d. The reaction is first order for X and zero order for Y and k=-3.35x10-2 M-1s-1 e. The reaction is first order for both X and Y and k=-3.35x10-2 M-1s-1 Using the information in the question above, if X and Y both have initial concentrations of 0.10M, what will the concentration of X be after 75 seconds?
Want solution asap
8. Dinitrogen tetraoxide (N2O4) decomposes spontaneously at room temperature in the gas phase: N2O4 (g) → 2 NO2(g) The rate law governing the disappearance of N2O4 with time is A[N,O4] = k N2O4]. At At 30°C, k = 5.1 x 106 s-1 and the activation energy for the reaction is 54.0 kJ/mol. Calculate the time (in seconds) required for the partial pressure of N2O4(g) to decrease from а. 0.10 atm to 0.010 atm at 30°C. b. Calculate the value of the rate constant at 300K. Repeat the calculation for the reaction in a) at the new temperature (300K). С. d. Write an observation about how the rate of reaction changed upon increasing the temperature.
X Cut AaBbCcl AaBbCcDc AaBbCcD AaBbCcE AaB AaBb CcC Aa8be T No Spac. Heading 2 Calibri (Body) | AA Aa. E , 刻T Copy Paste Subtle Title Subtitle BIU abc x, x A - y- A- Heading 1 T Normal Format Painter Paragraph Styles Font Clipboard I 10 11 6. From the data variation of the reaction rate of the following temperatures: 1500 T (K) k (M1 second ) 500 1000 5,49 x 106 9,86 x 108 5,09 x 10° Specify: a. Amount of Activation Energy (Ea) b. Magnitude of the pre-exponential factor (A)
At a temperature of 27oC and the reaction rate is 6.378 x 10-1 s-1. The reaction is of order 1. It has an activation energy (Ea) of 49884 J/mol and R = 8.314 J/mol.K, at a temperature of 127 oC the reaction rate constant is……… A. 1B. 100C. 10D. 1000E. 0.1
What is the order of the reaction with respects to B and why is that? Please explain .
General Chemistry II- Ara Sinavi 13 According to the data given below calculate k and t1/2. For the hypothetical aqueous reaction: A B, the concentration change of A was monitored and several derived data were tabulated and two different plots were obtained. Based on these given plots and data: time(min) [A] (M) In[A] V [A] -0.2 0.65 -0.43 1.5 --0.4 10 0.51 -0.67 2.0 -0.6 S -0.8 20 0.42 -0.87 2.4 -1.0 30 0.36 -1.02 2.8 Карat
23 II. An experiment followed the decomposition. of nitregen dioxide to nitregen monoxide & oxygen gas. Given the following data, what order is the reaction for nitrogen dioxide? Given an initial concentration of nitrogen dioxide of 0.0400 M, what's the concentration of this reactant after a half hour? show all grapers & calcs to determine answers. (sec) Time |[NO₂] (M) 0.0 50.0 100.0 200.0 300.0 0.01000 0.00787 0.00649 0.00481 0.00380 M G 2 XX 6.5 Hoa X019 201 2(x) = 2 (1.86) (3 (9)

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS