At elevated temperatures, dinitrogen pentoxide decomposes oxygen: 2N₂O5 (9)→ 4NO2(9) + O2(g) nitrogen dioxide and ▾ Part A When the rate of formation of O₂ is 2.3x10-3 M/s, the rate of decomposition of N₂O5 is O 4.6-10-3 O 5.8x10-4 O 23x10-3 O 12x10-3 O 9.2×10-3 Submit Provide Feedback Request Answer M/s. R

At elevated temperatures, dinitrogen pentoxide decomposes oxygen: 2N₂O5 (9)→ 4NO2(9) + O2(g) nitrogen dioxide and ▾ Part A When the rate of formation of O₂ is 2.3x10-3 M/s, the rate of decomposition of N₂O5 is O 4.6-10-3 O 5.8x10-4 O 23x10-3 O 12x10-3 O 9.2×10-3 Submit Provide Feedback Request Answer M/s. R

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

Suppose you are studying the kinetics of the reaction between nitrogen monoxide and hydrogen gas. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 0.0050 0.0020 1.25 x 10–5 2 0.010 0.0020 5.00 x 10–5 3 0.0050 0.0040 2.50 x 10–5 Based on the data, choose the correct exponents to complete the rate law. rate=k[NO]x[H2]y x=? y=?
The decomposition of N₂O5 proceeds according to the following equation: 2N2O5 (g) → 4NO₂(g) + O₂(g) If the rate of decomposition of N₂O5 at a particular instant in a reaction is 4.2 x 10-7 M/s, what is the rate of formation of O₂? Show work.
٩
For the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C, the rate of the reaction is determined by measuring the appearance of O2. 2 N2O54 NO2 + O2 At the beginning of the reaction, the concentration of O2 is 0 M. After 183 min the concentration has increased to 0.380 M.What is the rate of the reaction? (mol O2/L) /min
Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.
Some measurements of the initial rate of a certain reaction are given in the table below. [N-] |H2 initial rate of reaction 4 0.185 M 0.675 M 3.00 x 10“M/s 0.185 M 1.34M 1.18 x 10°M/s olo 0.236M 0.675M 3.83 × 10*M/s Ar Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate k x10 k =
In a study to determine the rate of the following reaction: $$2NO(g)+O2(g) 2NO2(g) the concentration of NO was 0.0400 M at t = 5.0 s and 0.0225 M at t = 650.0 s. What is the average rate of the reaction during this time period?
2NOCl(g) → 2NO(g) + Cl2(g) Rate = k[NOCl]2If this gaseous system has an initial rate of decomposition of NOCl of 0.0010 M s-1, and the volume of the system is reduced to one fifth of its original value, what is the new initial rate of decomposition of NOCl? Assume the temperature remains the same. 5.0×10-3 M s-1 2.5×10-2 M s-1 2.0×10-4 M s-1 4.0×10-5 M s-1 1.0×10-1 M s-1
Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: Part A 2NO2 (g) → 2NO(g) + O2(g) In a particular experiment at 300 °C, [NO2] drops from 0.0100 to 0.00750 M in 100 s. The rate of appearance of O2 for this period is M/s. 5.0 x 10-5 1.3 x 10-5 2.5 x 10-3 5.0 x 10-3 2.5 х 10 5
At 10°C , if rate of a chemical reaction is X M/s ,then at 20°C, the rate will almost be equal to O 10X 3X O 4X O 2X
Sulfur trioxide production follows the reaction: 2 SO2(g) + O2g) → 2 SO3(g) If the rate at which SO3 is produced is 4.28 x 10-4 mol L-'s-1, at what rate is SO2 consumed? A 4.28 x 10-4 mol L-'s-1 B 1.07 x 10-4 mol L-'s-1 2.14 x 10-4 mol L-'s-1 1.08 x 10-3 mol L-'s-1
A chemistry graduate student is studying the rate of this reaction: 2H1 (g) - H₂ (g) +1₂ (g) She fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [HI] 1.00 M 0.227M 0.20 0.128M 0.30 0.0894M 0.40 0.0686M Use this data to answer the following questions. Write the rate law for this reaction. 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=& D.D