B. ConcentrationTable B: Reaction Rate of Na S O/HCIBeaker #12345A-Volume-of 0.15 MNa,S,O, (aq)used / ml.50.040.030.020.010.0B-Volume ofwater/mL.0.010.020.030.040.0Totalvolume(A+B)/ml50.050,050.050.050.0*Concentration ofNa,8,0, (aq)/mol L15.12090060030Plot two graphs:1. Time vs concentration of Na.S,O, (aq)2. 1/Time vs concentration of Na S.O, (aq)Time/s22.527.335.160.0159.1Explain the observations (relationship between concentration and time).1/time/04440366*Use civic₂V; to determine the concentration of the diluted sodium thiosulphate solution(beakers 2-5). On how to use this dilution formula, then, please watch:0285016700629

Concentration of solution usually tells about the quantity of solute added in solvent to form…

Table B: Reaction Rate of Na S O/HCI A-Volume of 0.15 M Na S,O, (aq) used / ml. 50.0 40.0 30.0 Beaker # 12345 20.0 10.0 B- Total Volume of volume water/mL. (A+B) /ml 50.0 50.0 50.0 0.0 10.0 20.0 30.0 40.0 50.0 50.0 *Concentratio n of Na,S,0, (aq) /mol L 15 12 Plot two graphs: 1. Time vs concentration of Na S,0, (aq) 2 1/Time vs concentration of Na S,O, (aq) 090 060 030 Time/s 22.5 27.3 35.1 60.0 159.1 Explain the observations (relationship between concentration and time). 1/time/ st Use civicV; to determine the concentration of the diluted sodium thiosulphate solution (beakers 2-5). On how to use this dilution formula, then, please watch: 0444 0366 0285 0167 00629

Table B: Reaction Rate of Na S O/HCI A-Volume of 0.15 M Na S,O, (aq) used / ml. 50.0 40.0 30.0 Beaker # 12345 20.0 10.0 B- Total Volume of volume water/mL. (A+B) /ml 50.0 50.0 50.0 0.0 10.0 20.0 30.0 40.0 50.0 50.0 *Concentratio n of Na,S,0, (aq) /mol L 15 12 Plot two graphs: 1. Time vs concentration of Na S,0, (aq) 2 1/Time vs concentration of Na S,O, (aq) 090 060 030 Time/s 22.5 27.3 35.1 60.0 159.1 Explain the observations (relationship between concentration and time). 1/time/ st Use civicV; to determine the concentration of the diluted sodium thiosulphate solution (beakers 2-5). On how to use this dilution formula, then, please watch: 0444 0366 0285 0167 00629

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...

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Question

B. Concentration
Table B: Reaction Rate of Na S O/HCI
Beaker #
12345
A-Volume-
of 0.15 M
Na,S,O, (aq)
used / ml.
50.0
40.0
30.0
20.0
10.0
B-
Volume of
water/mL.
0.0
10.0
20.0
30.0
40.0
Total
volume
(A+B)
/ml
50.0
50,0
50.0
50.0
50.0
*Concentratio
n of
Na,8,0, (aq)
/mol L
15
.12
090
060
030
Plot two graphs:
1. Time vs concentration of Na.S,O, (aq)
2. 1/Time vs concentration of Na S.O, (aq)
Time/s
22.5
27.3
35.1
60.0
159.1
Explain the observations (relationship between concentration and time).
1/time/
0444
0366
*Use civic₂V; to determine the concentration of the diluted sodium thiosulphate solution
(beakers 2-5). On how to use this dilution formula, then, please watch:
0285
0167
00629

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2A(g) + 3/2B(g) Experiment e b) D d) k= 12345 Initial rate (mol/L.s) →→ C(g) 0.25*10-4 2.25x10-4 0.50×10-4 1.00×10-4 0.75*10-4 Initial [A] (mol/L) 5x10-2 15x10-2 5x10-2 10×10-2 5x10-2 unit: Overall reaction order is Rate = K[A][B] Initial [B] (mol/L) Reaction order with respect to A is Reaction order with respect to B is 5x10-2 5x10-2 10x10-2 5x10-2 15x10-2 O " O Calculate rate constant (k) based on data from experiment 3:
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Reaction Conc. Na2S½O3 Conc. HCI A Abs. A Time (s) Rate (A Abs./ga Time) 1.007568 0.300349 0.01870913 0.02870913 1 0.10 M .30 М 1.3686611 1.358380874 0.10 M .15 M 1.5360817 5.114311671 3 0.050 M .30 M 1.2267196 65.56796601 4 0.025 M .30 M 0.9563164 11.3085840 4. Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. The rate law of the reaction is shown below: Rate = [Na2S2O3]-2