Consider the reaction 2H3PO4→P2O5+3H2O Using the information in the following table, calculate the average rate of formation of P2O5 between 10.0 and 40.0 s. Time (s) 0 10.0 20.0 30.0 40.0 50.0 [P2O5] (M) 0 1.20×10−3 4.20×10−3 6.00×10−3 7.20×10−3 7.80×10−3 Express your answer with the appropriate units.

7. The rate of the reaction NO,(g) + CO(g) → NO(g) + CO,(g) depends only on the concentration of nitrogen dioxide below 225°C. At a temperature below 225°C, the following data were collected: Time (s) [NO,] (mol/L) 0.500 1.20 X 103 3.00 X 103 0.444 0.381 4.50 X 103 0.340 9.00 X 103 0.250 1.80 X 104 0.174 Determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [NO2] at 2.70 × 10* s after the start of the reaction.

Consider the reaction A⟶ Products. The rate law for this reaction is rate = k[A]2 where k=2.90 ×10-2 M-1s-1 at a particular temperature. If the initial [A] = 0.0500 M, what is the value of the half-life? 34.5 s 23.9 s 478 s 690. s

A study of the rate of the reaction represented as X + Y → 2 Z gave the following data: Time (s) 0.0 10.0 20.0 30.0 [A] (M) 0.8324 0.7115 0.6193 0.5463 Determine the average rate of disappearance of X between 20.0 s and 30.0 s, and the rate of appearance of Z between 20.0 and 30.0 s. 1) Average rate of disappearance of X between 20.0 s and 30.0 s = _______ M/s.   2) Average rate of appearance of Z between 20.0 s and 30.0 s = ______ M/s.

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Some measurements of the initial rate of a certain reaction are given in the table below. [N-] N2 H2 initial rate of reaction 0.556M 1.54M 6.00 × 10°M/s 0.181 M| 1.54M 1.95 × 10°M/s 0.556M 2.66M 1.79 × 10°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 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k U x10 k =

A chemistry graduate student is studying the rate of this reaction: 2C1,0, (3) – 2Cl, (g) +50, (g) She fills a reaction vessel with Cl,0, and measures its concentration as the reaction proceeds: time [CLO,] (seconds) 1.00 M 10. 0.666 M 20. 0.443 M 30. 0.295 M 40. 0.196 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k O Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.

Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.81M 0.376M 105 M/s 1.81M 0.0561 M 1.19 × 105 M/S 0.236M 0.376M 1.36 × 104 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 = k0.0² 0 8.00 × k = x10 0.0 X

A chemistry graduate student is studying the rate of this reaction: NH4OHaq→NH3aq+H2Oaq She fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds time(seconds) NH4OH 0 0.0700M 10. 0.0370M 20. 0.0196M 30. 0.0103M 40. 0.00547M 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 2significant digits. Also be sure your answer has the correct unit symbol. =k

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.