2H2O2(aq) → 2H2O(l) + O2(g) This reaction is first order, with a half life of 1455 seconds. What is the instantaneous rate of H2O2 decomposition, when [H2O2] = 0.25 M? 2.4×10-4 M s-1 1.2×10-4 M s-1 4.8×10-4 M s-1 6.0×10-5 M s-1 1.7×10-4 M s-1

The first-order reaction: S02CI2 → SO2 + Cl2 has a rate constant equal to 2.20 x 10-5 s-1 at 593 K. What percentage of the initial amount of SO,Cl2 will remain after 22.3 hours? 92.8 % 85.4 % O 1.00 % 17.1 % 14.7 %

Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0028 M.s¯¹: 2N₂O(g) 2N2(g) + O2(g) Suppose a 350. mL flask is charged under these conditions with 400. mmol of dinitrogen monoxide. After how much time is there only 200. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. X ☐ x10

The following reaction was studied at a given temperature: CH3CI(g) + H20(g) → CH3OH(g) + HCI(g) From the rate data below, determine the reaction orders. Exp [CH3CI]o [H2O]o Initial Rate (M s1) 1 0.100 0.100 0.182 2 0.200 0.200 1.45 3 0.200 0.400 5.81 CH3CI: first order H2O: first order CH3CI: second order H,O: second order CH3CI: second order H,O: first order O CH3CI: first order H2O: second order

The reaction N2O5- 2NO2 + 1/2 O2(g) is first order. The rate constant k is 6.2 x 10-4/min. A) What is the half life of this reaction in seconds and days? B) How long will it take for the concentration of N2O5 to decrease to 25% of it's original concentration?

Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0039 M²s¯¹: 2N₂O(g) 2 N₂(g) + O₂(g) Suppose a 4.0 L flask is charged under these conditions with 400. mmol of dinitrogen monoxide. How much is left 6.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 00 X 3

The rate law for the reaction is below: rate = k[IO3 ]²[SO3²]⁹ What is the meaning of the coefficients p and q in the reaction? They represent the coefficients in the balanced equation. They represent the rate each compound is used. They represent the charge on the ions. They represent the order of reaction with respect to each reactant.

A chemistry graduate student is studying the rate of this reaction: NH₂OH(aq) → NH3 (aq) +H₂O (aq) She fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds: time (milliseconds) 0 [NHẠOH] 0.0400M 10. 0.0126M 20. 0.00748M 30. 0.00532 M 40. 0.00413 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 X Ś

The first-order reaction, SO2C12 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2C12 will remain after 9.2 hours? 100% 99.9% 3.88% 48.3% 2.20%