A study of the rate of the reaction represented as 2 A B gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 35.0 [4] (M) 1.00 0.775 0.625 0.465 0.360 0.285 0.230 Determine the average rate of disappearance of A between 10.0 s and 20.0 s. 0.0652 mol L-1s-1 0.0562 mol L-1s-1 0.0265 mol L-1s-1 0.265 mol L-1 s-1

A study of the rate of the reaction represented as 2 A B gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 35.0 [4] (M) 1.00 0.775 0.625 0.465 0.360 0.285 0.230 Determine the average rate of disappearance of A between 10.0 s and 20.0 s. 0.0652 mol L-1s-1 0.0562 mol L-1s-1 0.0265 mol L-1s-1 0.265 mol L-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

Please don't provide handwritten solution ...
Initial rates were measured for the following reaction and are listed in the table. A + 2B ⎯→ products Expt. Initial Concentrations Initial Rate (mol/L·s) [A] [B] 1 0.115 0.135 2.70 × 10−3 2 0.115 0.270 2.16 × 10−2 3 0.345 0.135 8.10 × 10−3 What is the order of the reaction with respect to A, with respect to B, and overall?
A study of the rate of the reaction represented as 2 A → B gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 [A] (M) 1.00 0.776 0.603 The instantaneous rate for the reaction at t = 10.0 s is 30.0 0.468 0.363 0.282 0.219 M/s.
Consider the reaction and the information in the table provided. Calculate the average rate of formation of P2O5 between 20.0s and 40.0s. 2H3PO4 → P2O5 + 3H2O Time (s) 0.0 10.0 20.0 30.0 40.0 50.0 Conc P2O5 (M) 0 0.00120 0.00420 0.00600 0.00720 0.00780
Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.
6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179
: Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.30 0.20 Rate (mol/L/h) 8.0 x 10-10 3.2 x 10-9 7.2 x 10-9
Determine the (a) rate law (b) solve for the order, and (c) value of rate constant for the reaction. C + D + E ⟶⟶ Products Reaction # [C]0 [D]0 [E]0 Initial rate (mol/L s) 1 0.400 0.300 0.560 7.14 x 10 -4 2 0.100 0.500 0.200 4.55 x 10 -5 3 0.100 0.200 0.200 4.55 x 10 -5 4 0.400 0.300 0.750 1.28 x 10 -3 5 0.100 0.300 0.560 3.57 x 10 -4
Some measurements of the initial rate of a certain reaction are given in the table below. [N] [H] initial rate of reaction 0.957 M 2.07M 0.296 M/s 0.241 M 2.07M 0.0188 M/s 0.957 M 4.24M 0.606 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 2 significant digits. Also be sure your answer has the correct unit symbol. rate= k = ☐ x10 On ロ・ロ ☐ G
Consider the reaction: A + B --> products. From the following data obtained at a certain temperature, determine the order of the reaction (rate law) and calculate the rate constant: [A] (M) [B] (M) Rate (M/s) 1.50 1.50 3.15 X 10-1 1.50 2.50 2.98 X 10 –1 3.00 1.50 5.50 X 10-1
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCII → OI¯ + Cl¯ This rapid reaction gives the following rate data: |[OCI¯] (M) [I¯] (M) Initial Rate (M/s) 1.36 × 10-4 1.5 × 10- -3 3.0 × 10-³ 1.5 x 10- -3 1.5 x 10 -3 1.5 × 10-³ 3.0 × 10-³ 2.72 × 10-4 2.72 × 10-4 Calculate the rate constant with proper units. Express the rate constant to two significant figures. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash (e.g. ft * lb or ft-lb). k Submit Part C HÅ Value Request Answer Units ? Calculate the rate when [OC] = 2.3 × 10-³ and [I¯] = 6.0 × 10-4 Express the rate in molarity per second to two significant figures.