Dinitrogen pentoxide decomposes via a first order reaction. Rate = k[N,O5], k= 6.93 × 10-3 s-1 The concentration of N,O5 is initially 0.700 mol/L. After 100 s it has dropped to 0.350 mol/L and after 200 s it has dropped to 0.175 mol/L. What is the concentration after 150 s? HOW DO WE GET THERE? Use the first order concentration-time equation to determine [N2O5] remaining after 150 s. [N2O5] = 150 X mol/L

Dinitrogen pentoxide decomposes via a first order reaction. Rate = k[N,O5], k= 6.93 × 10-3 s-1 The concentration of N,O5 is initially 0.700 mol/L. After 100 s it has dropped to 0.350 mol/L and after 200 s it has dropped to 0.175 mol/L. What is the concentration after 150 s? HOW DO WE GET THERE? Use the first order concentration-time equation to determine [N2O5] remaining after 150 s. [N2O5] = 150 X mol/L

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

The decomposition of N,Os to NO, and O, is first order, with a rate constant of 4.80 x 10“/s at 45°C. If the initial concentration of N,O, is 2.89x102 mol/L, what is the concentration of N,05 after 452 s? How long would it take for the concentration of N,O5 to decrease to 1.00 x 10-² mol/L from an initial concentration of 2.89×102 mol/L? mol/L S Submit Show Tutor Steps
Consider the reaction, P4(g) + 10 Cl2(g) → 4 PCl5(g) The rate of the overall reaction is equal to 0.928 M/min. Fill in the blanks below so that the rate with respect to each species is equal to the overall rate. x = y = z =
A balloon has a volume of 4.44 Liters when it is at standard pressure and 48 degrees Celsius. What will its new volume be at standard temperature and 0.23 atm?
Dinitrogen pentoxide, N2O5, decomposes by a first order reaction with an activation energy of 110 kJ/mol. At 65 °C, the rate constant is k = 5.2 x 103 s1. 8.01 g of N2O5 is confined in a 0.75 liter container. After 1 minute, what is the concentration of N205? A. 0.001 M B. 0.0035 M C. 0.0724 M D. 6.33 x 10-2 M E. None of the above
The reaction I (ag) + OCI (ag) → IO (ag) + Cl¯(aq) was studied, and the following data were obtained: I]o (mol/L) [OCI¯], (mol/L) Initial Rate (mol/L · s) 0.080 0.14 7.90 x 10-2 0.040 0.14 4.00 x 10–2 0.020 0.070 9.90 × 10–3 -2 0.16 0.070 7.90 x 10 What is the rate law? (Use k for the rate constant.) Rate = Calculate the value of the rate constant. k = L/mol · s Calculate the initial rate for an experiment where both I and OCI are initially present at 0.14 mol/L. Rate = mol/L · s
Sulfuryl chloride, SO2 Cl2, decomposes when heated. So, Cl2 (g) → SO2 (9) + Cl2 (9) In an experiment, the initial concentration of SO, Cl, was 3.74 x 10-2 mol L. If the rate constant is 2.2 x 10-5/s, what is the concentration of S0, Cl, after 6.0 hr? The reaction is first order. Concentration = mol/L
A study of the rate of the reaction represented as X + Y → 2 Z gave the following data: Time (s) 0.0 10.0 20.0 30.0 [A] (M) 0.8324 0.7115 0.6193 0.5463 Determine the average rate of disappearance of X between 20.0 s and 30.0 s, and the rate of appearance of Z between 20.0 and 30.0 s. 1) Average rate of disappearance of X between 20.0 s and 30.0 s = _______ M/s. 2) Average rate of appearance of Z between 20.0 s and 30.0 s = ______ M/s.
A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) → 2SO₂ (g) + O₂ O₂(g) She fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds: time [SO3] (seconds) 0 0.800M 0.10 0.384M 0.20 0.252M 0.30 0.188M 0.40 0.150M Use this data to answer the following questions. Write the rate law for this reaction. x10 Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 ☐•☐ × Ś ? allo Ar 8 K
In a study to determine the rate of the following reaction: 2NO(g) + O₂(g) - 2NO₂(g) the concentration of NO was 0.0550 Mat t= 5.0 s and 0.0225 Mat t= 650.0 s. What is the average rate of the reaction during this time period? M/S
For the decomposition of nitrous oxide at 565 °C , the rate of the reaction is determined by measuring the appearance of O2. 2 N2O 2 N2 + O2 At the beginning of the reaction, the concentration of O2 is 0 M. After 18.5 min the concentration has increased to 0.183 M.What is the rate of the reaction? (mol O2 /L) / min
For the reaction of : 2 H2O2 (g) → 2 H2O (g) + O2 (g), consider this data table, What is the average rate of reaction between 40 and 50 s for hydrogen peroxide? Time (s) H2O2 (M) 0 1.000 10 0.747 20 0.561 30 0.403 40 0.298 50 0.214 -0.0084 M/s 0.0042 M/s 0.0168 M/s 0.214 M/s 0.0084 M/s
The decomposition of sulfuryl chloride, SO2Cl2, to sulfur dioxide and chlorine gases is a first-order reaction. It is found that at a certain temperature, the rate constant equals 9.19 × 10-6 s-1. How long will it take to decompose SO2Cl2 so that 30.0% remains? The starting concentration is 0.0217 M.