The decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C\[ \text{N}_2\text{O}_5 \rightarrow 2 \text{NO}_2 + \frac{1}{2} \text{O}_2 \]is **first order** in \(\text{N}_2\text{O}_5\) with a rate constant of \(4.10 \times 10^{-3} \, \text{min}^{-1}\).If the initial concentration of \(\text{N}_2\text{O}_5\) is \(0.594 \, \text{M}\), the concentration of \(\text{N}_2\text{O}_5\) will be \(\_\_\_\_\_\) M after 433 minutes have passed.

Given, N2O5 ----> 2NO2 + 1/2 O2 Reaction follows is first order kinetics. Rate constant (k) =…

The decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N₂O5 2 NO₂ + 12 0₂ is first order in N₂O5 with a rate constant of 4.10x10-³min-¹. If the initial concentration of N₂O5 is 0.594 M, the concentration of N₂O5 will be M after 433min have

The decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N₂O5 2 NO₂ + 12 0₂ is first order in N₂O5 with a rate constant of 4.10x10-³min-¹. If the initial concentration of N₂O5 is 0.594 M, the concentration of N₂O5 will be M after 433min have

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 nitramide in aqueous solution at 25 °c NH2NO2(aq)N½O(g) + H20(1) is first order in NH2NO2. During one experiment it was found that when the initial concentration of NH2NO2 was 0.402 M, the concentration of NH2NO2 dropped to 7.40x10-2 M after 25187 s had passed. Based on this experiment, the rate constant for the reaction is s-1.
The decomposition of nitramide in aqueous solution at 25 °C NH,NO,(aq)→N,0(g) + H,0(I) is first order in NH,NO,. During one experiment it was found that when the initial concentration of NH, NO, was 0.302 M, the concentration of NH,NO, dropped to 0.0507 M after 24805.0 s had passed. Based on this experiment, the rate constant for the reaction is
1 A first-order decomposition reaction has a rate constant of 0.00428 yr What is the half-life of the reaction? Round your answer to 3 significant figures. yr x10 × Ś
The decomposition of N2Os is first order and the rate constant k 6.82 X 103 s1. 2 N20s (g)> 4 NO2 (g) + 02 (g) at 70 °C. If the initial amount of N20s in a 2.0 L vessel is 0.0250 mol, determine the time in minutes it takes for the quantity of N20s to drop to 0.010 mol a. b. What is the half-life of N20s at 70 °C?
The decomposition of N,O5 to NO, and O, is first order, with a rate constant of 4.80 x 1o4/s at 45°C. If the initial concentration of N,O5 is 4.18×102 mol/L, what is the concentration of N205 after 548 s? How long would it take for the concentration ofN,O5 to decrease to 1.00 x 10-2 mol/L from an initial concentration of 4.18x102 mol/L?
The decomposition of nitrous oxide at 565 °C N,0(g)N2(g) +½ O2(g) is second order in N2O with a rate constant of 1.10x10-3 M's. If the initial concentration of N20 is 2.08 M, the concentration of N,0 will be |M after 3.30x103 seconds have passed.
The decomposition of nitrous oxide at 565 °CN2O(g)N2(g) + ½ O2(g)is second order in N2O with a rate constant of 1.10×10-3 M-1 s-1.If the initial concentration of N2O is 2.22 M, the concentration of N2O will be 0.258 M after seconds have passed.
The rate law for the decomposition of ozone to molecular oxygen 2 03(g) → 3 0₂ (9) is rate= k- [03]² [0₂] The mechanism proposed for this process is 03 0+0₂ k_₁ 0 +03 20₂ Derive the rate law from these elementary steps. Clearly state the assumptions you use in the derivation.
The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+½O₂(g) 1 is second order in N₂O with a rate constant of 1.10 × 10-³ M s If the initial concentration of N₂O is 2.16 M, the concentration of N₂O will be M after 1480 seconds have passed.
The gas phase decomposition of sulfuryl chloride at 600 K SO₂ Cl₂ (g) → SO₂ (g)+ Cl₂ (g) is first order in SO₂ Cl2 with a rate constant of 2.80 × 10-³ min-¹. If the initial concentration of SO₂ Cl2 is 0.00164 M, the concentration of SO₂ Cl2 will be 0.000364 M after min have passed.
NOBr(g) decomposes to form NO and Br2 by the reaction 2 NOBr(g) + 2 NO(g) + Br2(8) It is found that the reaction is second order in NOBr. The rate constant has been found to be 0.170 M-1 s1. In a situation where the initial concentration of NOBr in a vessel is 0.690 M, how long will it take for the concentration of Br2 to reach 0.180 M? (Assume, of course, that there was no Br in the vessel to begin with.) Report your result in seconds with one decimal place but do not put units in the