At a certain temperature the rate of this reaction is second order in N₂O5 with a rate constant of 19.6M¯¹.s¯¹: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) Suppose a vessel contains N₂O5 at a concentration of 0.980 M. Calculate the concentration of N₂O5 in the vessel 0.690 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. 0 X

Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +03 (g) → NO3 (g) + O₂(g) 2 NO3 (g) + NO₂ (g) → N₂O5 (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. rate = k rate constant k₁ k₂ ロ→ロ X Ś

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0041 M's : 2 HI(g) → H2(g)+I,(g) Suppose a 4.0 L flask is charged under these conditions with 300. mmol of hydrogen iodide. After how much time is there only 150. 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. x10

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0092 M-s : 2 HI (g) - H, (g) +L, (g) Suppose a 450. mL flask is charged under these conditions with 150. mmol of hydrogen iodide. After how much time is there only 75.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. dlo x10 8. 미

Under certain conditions the rate of this reaction zero order in dinitrogen monoxide with a rate constant of 0.0064 M · s: 2N,0 (g) – 2N, (g) +0, (g) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of dinitrogen monoxide. How much is left 5.0 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.

A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 2.55 x 108 s at 25°C. What is the half-life for the degradation of DDT in this experiment, in years? (1 year = 365 days) Round your answer to 2 decimal places.

The reaction of NOBr(g) to form NO(g) and Br2(g) is second order: 2NOBr(g) → 2NO(g) + Br₂(g) The rate constant is 0.556 L mol-¹ s¹ at some temperature. If the initial concentration of NOBr in the container is 0.21 M, how long will it take for the concentration to decrease to 0.028 M? t = S

At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.75Ms H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.130M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.0286 M. You may assume no other reaction is important. Round your answer to 2 significant digits. X ? S

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0069 M · s¯¹: 2 HI(g) → H₂(g) +1₂(g) Suppose a 5.0 L flask is charged under these conditions with 400. mmol of hydrogen iodide. How much is left 3.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. 0 00 X x10 ? olo Ar

The following reaction was studied at 25°C. The following results were obtained. a) What is the rate law for this reaction at this temperature? b) What is the value of the rate constant? Be sure to include the correct units in your answer.