Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0076 M's ': 2 NH, (g) → N2 (g) + 3 H, (g) Suppose a 5.0 L flask is charged under these conditions with 500. mmol of ammonia. 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. olo

Consider this reaction: 2HI (g) → H₂ (g) + 1₂ (g) At a certain temperature it obeys this rate law. rate = (0.00315 M¹-s¯¹) [HI] ² S olo Suppose a vessel contains HI at a concentration of 1.16M. Calculate the concentration of HI in the vessel 970. seconds later. You may assume no other reaction is important. Ar Round your answer to 2 significant digits. M x10 X Ś ?

Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0032 M's : 2 NH, (g) → N2 (g) +3 H, (g) Suppose a 3.0 L flask is charged under these conditions with 400. mmol of ammonia. How much is left 10. s later? You may assume no other reaction is important. olo Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. Ar

Consider this reaction: 2HI (g) → H₂(g) + 12₂ (8) At a certain temperature it obeys this rate law. rate = (0.0257 s¹) [HI] S d Suppose a vessel contains HI at a concentration of 0.180M. Calculate how long it takes for the concentration of HI to decrease by 83.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. x10 X S ?

Measuring total pressure is a convenient way to monitor gas reaction: 2NOCl(g) → 2NO(g) + Cl2(g). The rate of the reaction depends on the concentration of the reactant, which is proportional to the partial pressure of the reactant. Derive a relation connecting its velocity above reaction with initial pressure, P0, and total pressure, Pt, at time t.(Hint: Assume the reaction is 2nd order. Make a table with initial (t0) and final values ​​(t) of the moles of NOCl, NO, and Cl2, and construct the ideal gas equations for both cases. Use the ideal gas equation for t0 so that calculate the initial concentration of NOCl and substitute this value into the equation of ideal gases for t)

Consider this reaction: 2NH, (g) → N, (g) +3H, (g) At a certain temperature it obeys this rate law. 2 rate = (0.0581 Ms)[NH,1 Suppose a vessel contains NH, at a concentration of 1.39M. Calculate the concentration of NH, in the vessel 70.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ?

At a certain temperature the rate of this reaction is second order in SO, with a rate constant of 4.02 M 's': 2S0, (g) → 2S0, (g) +0,(g) Suppose a vessel contains SO , at a concentration of 0.790 M. Calculate how long it takes for the concentration of SO, to decrease to 0.103 M. You may assume no other reaction is important. Round your answer to 2 significant digits.

For the reaction: 3X (g) + 5Y (g) a b. →2Z (g) + 4L (g) Express the rate of the reaction in terms of the change in concentration of each reactant and product with time. + ✪ [X] is decreasing by ◆ = When [Z] is increasing at 0.16 mol/L.s, show how fast is [X] decreasing. + unit is ◆

At a certain temperature the rate of this reaction is first order in NH3 with a rate constant of 0.354 s : 2NH3(g) → N₂ (g) + 3H₂(g) Suppose a vessel contains NH3 at a concentration of 0.380M. Calculate the concentration of NH3 in the vessel 2.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X

The decomposition of hydrogen peroxide is described by the equation: 2H₂O₂ (aq)-2H₂O(0) + O₂(g) The reaction is first order in H₂O₂. It takes 10.0 hours for the concentration of H₂O₂ to drop from 2.0 M to 1.0 M. How many hours are required for the concentration of H₂O₂ to drop from 0.80 M to 0.050 M? 15.0 40.0 50.0 30.0 20.0 OOOOO R