The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 623 K.

The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 617 K.

Chlorine oxide (CIO), which plays an important role in the depletion of ozone, decays rapidly according to the equation 2CIO(g) →→→ Cl₂(g) + O₂(g) - From the following data, determine the reaction order and calculate the rate constant of the reaction. Time (s) [CIO] (M) 2.91 x 103 8.11 × 10-6 3.64 x 10-3 5.77 × 10-6 4.37x103 4.48 x 10-6 5.10 x 10 3 3.66 x 10-6 5.83 x 10-3 3.09 x 10-6 Reaction order: O O 1 2 Rate constant: k = x 10 Ms (Enter your answer in scientific notation.)

For the reaction: 3 Ag  +  NO3–  +  4 H+  –––>  NO  +  2 H2O  +  3 Ag+ If the rate of disappearance of Ag is 0.0017 mol L–1 s–1, what is the rate of the appearance of water? For the 1st order reaction:   A ––> products,    assume the concentration of A falls to one-third of its original value after 150 seconds.  Calculate the rate constant and the half-life.

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

Calculate the half life, ty (in min) for the first order reaction, A - B, if the reaction is 12.2% complete in 17.7 minutes. Report your answer to THREE significant figures.

b Sulfuryl chloride undergoes first-order decomposition at 320.°C with a half-life of 8.75 h (k = 2.20 x 10-5 s1). So,Cl2(g) → SO2(g) + Cl2(g) If the initial pressure of S02CI2 is 791 torr and the decomposition occurs in a 1.25-L container, how many molecules of SO2CI, remain after 11.7 h? molecules SO2CI2

The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 613 K.

The decomposition of ethylene oxide (CH₂)2O(g) → CH4(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 631 K.