Consider the reaction 2H3PO4→P205 + 3H2O Using the information in the following table, calculate the average rate of formation of P205 between 10.0 and 40.0 s. Time (s) 10.0 20.0 30.0 40.0 50.0 [P2O5] (M) 0 1.40x10-3 4.40x10-3 6.20x10-3 7.40x10-3 8.00x10-3 Express your answer with the appropriate units. • View Available Hint(s) μΑ Rate of formation of P205 = Value Units Submit

Consider the reaction 2H3PO4→P205 + 3H2O Using the information in the following table, calculate the average rate of formation of P205 between 10.0 and 40.0 s. Time (s) 10.0 20.0 30.0 40.0 50.0 [P2O5] (M) 0 1.40x10-3 4.40x10-3 6.20x10-3 7.40x10-3 8.00x10-3 Express your answer with the appropriate units. • View Available Hint(s) μΑ Rate of formation of P205 = Value Units Submit

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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NO2(g) + CO(g) NO(g) + CO2(g) The rate of the above reaction depends only on the concentration of nitrogen dioxide at temperatures below 225°C.At a temperature below 225°C the following data were obtained: Time(s) [NO2](mol/L) 0 0.440 1.55×103 0.418 3.88×103 0.389 5.81×103 0.368 1.16×104 0.317 2.32×104 0.248 Which of the following expressions for the rate law (either differential or integrated) are completely consistent with the above experimental data. ln([NO2]/[NO2]0) = -kt [NO2] = [NO2]0 - kt d[NO]/dt = k[NO2] k[NO2]2 = d[CO2]/dt 1/[NO2] - 1/[NO2]0 = kt Calculate the rate constant (k). Enter the numerical value and corresponding units.
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
A chemistry graduate student is studying the rate of this reaction: 2C1₂05 (g) → 2Cl₂(g) +50₂ (g) She fills a reaction vessel with Cl₂O5 and measures its concentration as the reaction proceeds: time (minutes) 0 10. [CI,Os] 0.300M 0.161M 20. 0.0864M 30. 0.0464M 40. 0.0249M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = x10 0.0 X 5
For the reaction of : 2 H2O2 (g) → 2 H2O (g) + O2 (g), consider this data table, What is the average rate of reaction between 40 and 50 s for hydrogen peroxide? Time (s) H2O2 (M) 0 1.000 10 0.747 20 0.561 30 0.403 40 0.298 50 0.214 -0.0084 M/s 0.0042 M/s 0.0168 M/s 0.214 M/s 0.0084 M/s
For the reaction: NO2(g) → 1/2 O2(g) + NO (g) The following data were obtained: Time (s) 0 50 100 [NO₂] (M) 0.01 Concentration NO2 0.00787 -4.844697217 127.064803 200 0.00481 -5.337058195 0.00649 -5.037492748 154.0832049 300 0.0038 -5.572754212 0.012 0.01 0.008 Natural Log [NO2] (M) Determine the rate law of this reaction and the value of k, the rate constant. The graphs of the data appear below. 0.006 0.004 -4.605170186 100 0.002 0 0 1/[NO2] 100 200 Time (s) 207.9002079 1/[NO2] 263.1578947 y = -1.97E-05x + 9.15E-03 R² = 9.27E-01 300 250 200 150 100 50 0 300 0 50 400 100 Natural Log [NO2] 150 -4.5 -4.7 -4.9 -5.1 -5.3 -5.5 -5.7 0 200 Time (s) y = 0.5431x + 99.833 R² = 1 100 250 300 200 Time (s) 350 y = -0.0032x - 4.6679 R² = 0.9824 300 400
The reaction H2 (g) + 2 NO (g) + H,O (g) is studied at a certain temperature by determining the rate of reaction at reactant concentrations. The results are as follows: N,0 (g) 2. Concentration (M) Rate [NO] (i) (ii) [H] (M/s) 0.25 0.10 0.126 0.50 0.10 0.504 (iii) 0.50 0.20 1.03 The rate law is written as Rate = k [NO]* [H]°. The exponents x and y represent the order with respect to NO and H2, respectively. Calculate the value of x and y from the data provided.
The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]^ , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is M-1s-1.
A chemistry graduate student is studying the rate of this reaction: 2C1,0, (g)- 2C1, (g) +50, (g) He fills a reaction vessel with Cl,0, and measures its concentration as the reaction proceeds: time [C,0,] (seconds) 0| 0.0900 M 10. 0.0579 M 20. 0.0372 M 30. 0.0239 M 40. 0.0154 M Use this data to answer the following questions. Write the rate law for this reaction. rate Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
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: 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
A chemistry graduate student is studying the rate of this reaction: →H2CO3aq+H2OaqCO2aq She fills a reaction vessel with H2CO3 and measures its concentration as the reaction proceeds time(seconds) H2CO3 0 0.500M 10. 0.101M 20. 0.0563M 30. 0.0390M 40. 0.0298M Use this data to answer the following questions. Write the rate law for this reaction. rate =k Calculate the value of the rate constant k.Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. =k