The decomposition of dinitrogen pentoxide occurs by the following reaction.2 N2O5 - 4 NO2(g) + O₂(g)The experimentally determined rate law is Rate = k [N₂O5] and at this particulartemperature, the rate constant has the value 0.200 min-¹.When the concentration of N2O5 is 0.800 M, what is the rate of production ofNO2(g)?Report your answer in M min 1 but do not enter any units. Use three significantdigits.Your Answer:Your Answer 273.15 K = 0 °C NA = 6.02,RT/F = 0.025693 V (RT/F) In10 = 0.059160 V @ T = 298.15 KR = 8.3145 J K-1 mol-¹ = 0.082057 L atm K-1 mol-1F = 96,485.3 C/mol1 atm = 1.01325 bar = 760 Torr = 101325 Pa1023 mol-1

Answered: Image /qna-images/answer/d026eb01-2109-466a-8787-187f956423e9.jpg

The decomposition of dinitrogen pentoxide occurs by the following reaction. 2 N₂O5 4 NO2(g) + O2(g) - The experimentally determined rate law is Rate = k [N₂O5] and at this particular temperature, the rate constant has the value 0.200 min-¹. When the concentration of N₂O5 is 0.800 M, what is the rate of production of NO₂(g)? Report your answer im M min-¹ but do not enter any units. Use three significant digits. Your Answer: Your Answer

The decomposition of dinitrogen pentoxide occurs by the following reaction. 2 N₂O5 4 NO2(g) + O2(g) - The experimentally determined rate law is Rate = k [N₂O5] and at this particular temperature, the rate constant has the value 0.200 min-¹. When the concentration of N₂O5 is 0.800 M, what is the rate of production of NO₂(g)? Report your answer im M min-¹ but do not enter any units. Use three significant digits. Your Answer: Your Answer

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

5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
A chemistry graduate student is studying the rate of this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) She fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time [C1,05] (seconds) 0 0.400M 10. 0.263 M 20. 0.173 M 30. 0.114M 40. 0.0751M Use this data to answer the following questions. Write the rate law for this reaction. x10 Calculate the value of the rate constant k. X Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 Ś ?
: Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.30 0.20 Rate (mol/L/h) 8.0 x 10-10 3.2 x 10-9 7.2 x 10-9
The decomposition of ethyl chloride, CH3CH2Cl, follows the rate law: Rate = k[CH3CH2Cl]. At 550°C, k = 3.2 x 10-2 sec-1. What is the half-life for this reaction? What was the initial concentration of ethyl chloride if after one minute, 0.01 M remains?
13.102 Chlorine oxide (CIO), which plays an important role in the depletion of ozone (see Problem 13.101), decays rapidly at room temperature according to the equation 2C10(g) Cl₂(g) + O₂(g) From the following data, determine the reaction order and calculate the rate constant of the reaction. Time (s) 0.12 x 10-³ 0.96 x 10-³ 2.24 x 10-³ 3.20 x 10-³ 4.00 x 10-³ [CIO] (M) 8.49 x 10-6 7.10 x 10-6 5.79 x 10-6 5.20 x 10-6 4.77 x 10-6
Consider this reaction: 2HI (g) → H, (g) +I, (g) At a certain temperature it obeys this rate law. rate =(0,465 s)[HI Suppose a vessel contains HI at a concentration of 0.540M. Calculate the concentration of HI in the vessel 2.80 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Please complete the question typed ONLY. Please do not use handwriting.
2 3 4 =5 #1 6 7 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0040 M-s¹: 2 HI (g) → H₂(g) + 1₂ (g) Suppose a 5.0 L flask is charged under these conditions with 300. mmol of hydrogen iodide. How much is left 4.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. S A S ? Continue Submit 00 X
Ozone reacts with nitrogen dioxide to produce oxygen and dinitrogen pentoxide according to the following chemical equation: O3(g) + 2NO2(g)→ 02(g) + N2O5(g) The rate law for this reaction is Rate = k[O3]|NO2]. If concentration is measured in moles per liter and time is measured in seconds, what are the units of k?
The observed rate law for the reaction of nitrogen monoxide (NO) with chlorine (Cl₂) is: rate = K[NO]²[Cl₂] What is the overall reaction order? 00 0 1 O 2 O 3