The decomposition of gaseous dinitrogen tetraoxide (N2O5) to nitrogen dioxide and oxygen gases is a first order process with a rate constant of 0.0394 s-1 at a certain temperature. If the initial concentration of N2O5 (g) is 0.853 M, how long (in seconds) will it take for the concentration to reach 0.187 M? (answer in 3 signicicant figures )

The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 10-4 s-1. If the initial concentration of N2O5 is 0.11 M, what is its concentration after exactly 11 minutes have passed?   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

Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0037 M's : 2 N,0(g) 2 N2(g)+O,(g) Suppose a 5.0L 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 the correct number of significant digits.

4) The decomposition of phosphorus pentachloride (PCIS) into phosphorus trichloride (PCI3) and chlorine gas (Cl2) is a first order process with a rate constant of 0.0842 s at a certain temperature. If 40.4 s after the reaction begins, the concentration of PCIs is 0.0203 M, what was the initial concentration of PCI3? (A) 6.76 x 104 M (B) 0.609 M (C) 3.42 M (D) (E) 0.495 M ES 0.820 Mt (D)

4 At a certain temperature the rate of this reaction is first order in CICH₂CH₂Cl with a rate constant of 6.83 × 10 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) S Suppose a vessel contains CICH₂CH₂Cl at a concentration of 0.890M. Calculate the concentration of CICH₂CH₂Cl in the vessel 880. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

At a certain temperature the rate of this reaction is second order in CICH₂CH₂Cl with a rate constant of 0.00455 M S -1 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.11 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 900. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

The decomposition of N,O, in solution in carbon tetrachloride is a first-order reaction. 2N,O, → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 104 s'. If the initial concentration of N,O5 is 0.16 M, what is its concentration after exactly 13 minutes have passed?

Chlorine monoxide accumulates in the stratosphere above Antarctica each winter and plays a key role in the formation of the ozone hole above the South Pole each spring. Eventually, ClO decomposes according to the equation:  picture The second-order rate constant for the decomposition of ClO is 6.78×109 M–1s–1 at a particular temperature. Determine the half-life of ClO when its initial concentration is 1.46×10-8 M .

The first-order rate constant for the decomposition of N₂O5, given below, at 70°C is 6.82 x 10³ s¹. Suppose we start with 0.0500 mol of N₂O5(g) in a volume of 2.5 L. 2 N₂05(g) → 4 NO₂(g) + O₂(g) (a) How many moles of N₂O5 will remain after 3.0 min? mol (b) How many minutes will it take for the quantity of N₂O5 to drop to 0.005 mol? min (c) What is the half-life of N₂O5 at 70°C? min