Some measurements of the initial rate of a certain reaction are given in the table below [H _{2}]; [1_{2}] initial rate of reaction 0.254M 1.81 M 3 * 10 ^ 5* M/s 0.0345M 1.81M 4.07 * 10^4* M/s 0.254M 0.771 M 1.28 * 10 ^ 5* M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = kappa Box; Box x^ Box Box Box; x =

A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) → 2SO₂(g) + O₂(g) He fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds: time (minutes) 0 10. 20. 30. [so,] 0.0500M 0.0190M 0.0117 M 0.00847 M 40. 0.00663 M 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 = 0 x10 ロ・ロ X

Consider the given reaction : 2HgC2(ag) + C204²(ag) – 2CH(ag) + 2CO2(g) + Hg2Cl2(s) Experiment [HgCl2] [C2O42] Initial rate 1 0.0836 M 0.202 M 5.2 x10-5 0.0836 M 0.404 M 2.08 x10-4 0.0418 M 0.404 M 1.04 x104 4 0.0627 M 0.606 M ? Calculate the initial rate for experiment 4. 3.50 x 10-4 M min-1 8.75 x 103 M min-1 1.20 x 10-4 M min-1 O 6.00 x 104 M min 1

For the reaction 4 NH, (g) + 7 0, (g) → 4 NO,(g) + 6 H,(g), if H2 is produced at a rate of 3.5 x 10-3 M/s, Oz is consumed at a rate of -5.8 x 10-4 M/s. b. -2.1 x 10-2 M/s. -3.0 x 10-3 M/s. d. -2.5 x 10-2 M/s. -4.1 x 10-3 M/s. e. c.