A gas mixture was prepared at 500 K with total pressure 3.26 atm and a mole fraction of 0.00057 of ÑO and 0.00026 of O3. The elementary reaction NO + O3 → NO2 + O2 has a second-order rate constant of 7.6 × 107 L mol¬1 s- at this temperature. Calculate the initial rate of the reac- tion under these conditions.

A gas mixture was prepared at 500 K with total pressure 3.26 atm and a mole fraction of 0.00057 of ÑO and 0.00026 of O3. The elementary reaction NO + O3 → NO2 + O2 has a second-order rate constant of 7.6 × 107 L mol¬1 s- at this temperature. Calculate the initial rate of the reac- tion under these conditions.

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

For the reaction A--->B, the rate law is delta[B]/delta t=k[A]2. What are the units of rate constant where time is measured in seconds?
A compound with the formula, C3H6 undergoes an isomerization reaction in the gas phase to form a new compound with the same molecular formula. The isomerization reaction is first-order with a rate constant of 5.87 x 10-4 sec-1 at 485 degrees Celsius. If a 2.50 liter flask initially contains 722 torr of the starting gaseous compound at 485 degrees Celsius, how long will it take, in minutes, for the partial pressure of the starting compound to drop below 1.00 x 102 torr?
The hydroxyl radical in the atmosphere is most effectively removed by hydrocarbons such as methane according to the second-order reaction below. •OH + CH4 - H20 + CH3' Given that the second-order rate constant is 3.0x106 L·mol-1.s-1, calculate the lifetime of the radical at 19°C if the concentration of CH4 is 1.5×103 ppb by volume. (Hint: The lifetime of the radical is given by 1/k[CH4].) 4.0 3.6e-3 X S
At a given temperature, a first-order reaction has a rate constant of 1.5 × 10–3 s–1. What is the time required for the reaction to be 32% completed?
How do you find the order for [O2]?
The hydroxyl radical in the atmosphere is most effectively removed by hydrocarbons such as methane according to the second-order reaction below. •OH + CH4 - H20 + CH3: Given that the second-order rate constant is 3.0x106 L·mol-1.s-1, calculate the lifetime of the radical at 19°C if the concentration of CH4 is 1.5×103 ppb by volume. (Hint: The lifetime of the radical is given by 1/k[CH4].) 4.0 3.55e-3
The rate for the reaction H2 (g) + Br2 (g) 2 HBr (g)is first order in both H2 and Br2 concentrations, and the rate constant k at 287 \deg C is 5.87\times 10-4 L mol-1 s-1. Suppose 1.00 L of H2 (g) at a concentration of 6.60\times 10-2 M is rapidly mixed with the same volume of Br2 (g) also at a concentration of 6.60\times 10-2 M. Calculate the time (in seconds) required for the H2 concentration to decrease to a value of 2.55\times 10-2 M. (Enter your answer to three significant figures.)
At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.75Ms H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.130M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.0286 M. You may assume no other reaction is important. Round your answer to 2 significant digits. X ? S
Hydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation 2H,0, (aq) — 2н,00) + 0,(8) The activation energy for this reaction is 75 kJ-mol-1. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ-mol-1. At what temperature would the non-catalyzed reaction need to be run to have a rate equal to that of the metal-catalyzed reaction at 25 °C? T = K
Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction 2NO (g) → N₂O₂ (g) step 1 2 N₂O₂(g) + O₂ (g) Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. 2NO₂ (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. << Note: your answer should not contain the concentrations of any intermediates. rate constant 0 k₁ k₂ rate = k 1-0 010 X S