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 0.25 M, what is its concentration after exactly 6 minutes have passed?   Round your answer to 2 decimal places.

273.15 K = 0 °C NA = 6.02, RT/F = 0.025693 V (RT/F) In10 = 0.059160 V @ T = 298.15 K R = 8.3145 J K-1 mol-¹ = 0.082057 L atm K-1 mol-1 F = 96,485.3 C/mol 1 atm = 1.01325 bar = 760 Torr = 101325 Pa 1023 mol-1

The first-order reaction: S02CI2 → SO2 + Cl2 has a rate constant equal to 2.20 x 10-5 s-1 at 593 K. What percentage of the initial amount of SO,Cl2 will remain after 22.3 hours? 92.8 % 85.4 % O 1.00 % 17.1 % 14.7 %

The decomposition of compound XYZ is a 2nd order reaction. Initially, the concentration of XYZ was 2.80 M. If the rate constant of this reaction is 4.31 M-1 min-1. How many minutes are required for the concentration of XYZ to become 0.700 M? Your answer should have 3 significant figures.

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0188 s NH,OH (aq) → NH, (aq)+H,0 (aq) Suppose a vessel contains NH,OH at a concentration of 0.590M. Calculate the concentration of NH,OH in the vessel 49.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.00717 s : CICH,CH,CI (g) → CH,CHCI (g) + HCI (g) Suppose a vessel contains CICH,CH,Cl at a concentration of 1.00M. Calculate the concentration of CICH,CH,Cl in the vessel 89.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. |M Ox10 ?

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0424 s¯¹: S 2NH3(g) → N₂(g) + 3H₂(g) Suppose a vessel contains NH3 at a concentration of 0.460M. Calculate the concentration of NH3 in the vessel 17.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X 5

At a certain temperature this reaction follows first-order kinetics with a rate constant of  :0.0303s−1 →NH4OHaq+NH3aqH2Oaq Suppose a vessel contains  NH4OH  at a concentration of  0.410M . Calculate how long it takes for the concentration of  NH4OH  to decrease to  0.0492M . You may assume no other reaction is important. Round your answer to  2  significant digits.

Nitrosyl bromide decomposes by the reaction 2 NOBr(g) → 2 NO(g) + Br₂(g). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. Students may do this by plotting the data three different ways. For each plot, time goes on the x-axis. A zero-order reaction is linear when [NOBr] on the y-axis. A first-order reaction is linear when In [NOBr] is on the y-axis. A second-order reaction is linear when 1/[NOBr] is on the y-axis. t [NOBr] 0 0.0653 OM-2.5-2 O M-¹. S-1 What are the units for the rate law? O M-2. s-1 OM-3. s-1 5 15 50 10 85 0.0514 0.0424 0.0361 0.0177 0.0117 What is the rate law for the reaction? (Rate equations take the general form 'rate = k. [A] . [B]'.) What is the value of the rate constant at the temperature of the experiment? 4.0✔ S M chemPad XX⁰ ← → Help Greek

At a certain temperature this reaction follows second-order kinetics with a rate constant of 1.0M 2NH, (g) - N, (2) + 3H, (g) Suppose a vessel contains NH, at a concentration of 1.07M. Calculate how long it takes for the concentration of NH, to decrease by 91.%. You may assume no other reaction is important. Round your answer to 2 significant digits.