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, CIO decomposes according to the equation: 2C10 (g) > Cl₂(g) + O₂(g) The second-order rate constant for the decomposition of CIO is 6.48×10⁹ M-¹s-1 at a particular temperature. Determine the half-life of CIO when its initial concentration is 1.76×10-8 M. x 101

Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.0317 M¹-s¯¹) [₂0₂] S Suppose a vessel contains N₂O5 at a concentration of 0.440 M. Calculate the concentration of N₂O5 in the vessel 480. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ? X S

Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) +O₂ (g) At a certain temperature it obeys this rate law. rate = (0.0328 s−¹)[N₂05] S Suppose a vessel contains N₂O5 at a concentration of 0.860M. Calculate the concentration of N₂O5 in the vessel 22.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś

Consider following reaction:              2 A2B5(g)  →  4AB2(g) + B2(g) The rate constant is 0.129 s-1 at 298 K for this reaction. What is the percent of A2B5 left after the first 19.091 s? Report your answer with three decimals. Enter numbers only;

At a certain temperature the rate of this reaction is first order in HI with a rate constant of 1.13 s : 2HI (g) → H2 (g) +I, (g) Suppose a vessel contains HI at a concentration of 1.01 M. Calculate the concentration of HI in the vessel 0.730 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Ox10

The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N2O5 and first order overall.  The rate constant for the reaction at 70.oC is 6.82x10-3 s-1.  The reaction is started with 0.300 mol of N2O5 in a 0.500L container. How many minutes will it take for the concentration of N2O5 to drop to 0.145M?

A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O₂(g) + NO(g) →→→ O₂(g) + NO₂ (g) -> The rate law for this reaction is rate of reaction = k [0₂] [NO] Given that k = 4.78 × 106 M-¹.s¹ at a certain temperature, calculate the initial reaction rate when [03] and [NO] remain essentially constant at the values [03] = 7.59 × 10-6 M and [NO]。 = 6.45 × 10-5 M, owing to continuous production from separate sources. initial reaction rate: Calculate the number of moles of NO₂ (g) produced per hour per liter of air. NO₂ produced: M-s-1 mol-h-¹.L-1

The production of nitric oxide is governed by the reaction:   4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)   If the rate at which NO is produced is 6.35 × 10−2 mol L−1s−1, at what rate is O2 consumed

Consider the reaction for the formation of ammonia, NH3:                              N2(g) + 3 H2(g) --> 2 NH3(g) Which is the correct rate expression for this reaction?

The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) → ½ H2 (g) + ½ I2 (g) is zero order in HI with a rate constant of 1.20×10-4 M/s How much time is required for the concentration of HI to drop to 9.40×10-2 M if its initial concentration is 0.525 M?