The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N205 - 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 N205 is 0.28 M, what is its concentration after exactly 15 minutes have passed? Round your answer to 2 decimal places.

The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N205 - 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 N205 is 0.28 M, what is its concentration after exactly 15 minutes have passed? Round your answer to 2 decimal places.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

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
Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant 1 03(g) O₂(g) + 0(g) k₁ 2 03(g) + O(g) → 20₂(g) k₂ Suppose also k₁ »k₂. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K2, and (if necessary) the rate constants k.1 and k-2 for the reverse of the two elementary reactions in the mechanism. = 0 k = 00 X 5 S ?
The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 41 minutes. Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 0.35 µg/mL. What will the concentration be 123 minutes later? Round your answer to 2 significant digits. e ml. 0.8
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 ?
Please don't provide handwritten solution ....
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.
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.
The first-order reaction, SO2C12 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2C12 will remain after 9.2 hours? 100% 99.9% 3.88% 48.3% 2.20%
Your laboratory is asked to analyze a water sample for a particular pesticide. You know from previous study that this pesticide degrades via a first order, irreversible reaction. The first order rate constant (k) for the reaction at 4 °C is 0.02 day¹. The activation energy for the reaction is known to be 10 kcal/mol. The standard preservation method for water samples containing this pesticide is to store the sample at 4 °C for no more than 24 hours prior to analysis. Calculate the fraction of the pesticide that remains in the sample after 24 hours of storage at 4 °C. b. A newly hired staff member collects a sample of the water but forgets to store it at 4 °C. Instead, they leave the sample in the trunk of their car (average temperature 35 °C) over the weekend. 60 hours later the sample is analyzed and found to contain 0.01 mg/L of the pesticide. What was the pesticide concentration in the water at the time the sample was taken?