The reaction described by the equationO3 (g) + NO(g)0,(g) + NO,(g)has, at 310 K, the rate lawrate of reaction =k[O¸][NO]k = 3.0 x 106 M-1-s-!Given that [O,] = 8.0 x 10-4 M and [NO] = 3.0 x 10-3 M at t =:0, calculate the rate of the reaction at t = 0.rate:M/sWhat is the overall order of this reaction?3

Answered: Image /qna-images/answer/f0d2e85a-9d62-409c-ac20-3081d27884f1.jpg

The reaction described by the equation 0,(g) + NO(g) - 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O¸][NO] k = 3.0 × 10 M-'. 1.s-1 Given that [O,] = 8.0 × 10-4 M and [NO] = 3.0 × 10¬ M at t = 0, calculate the rate of the reaction at t = 0. rate: M/s What is the overall order of this reaction? 3 2 1

The reaction described by the equation 0,(g) + NO(g) - 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O¸][NO] k = 3.0 × 10 M-'. 1.s-1 Given that [O,] = 8.0 × 10-4 M and [NO] = 3.0 × 10¬ M at t = 0, calculate the rate of the reaction at t = 0. rate: M/s What is the overall order of this reaction? 3 2 1

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 rate of the reaction N₂O5(g) →2 NO₂(g) + 1/2 0₂(g) is measured at different temperatures, with the following rate constants, k, determined: Temperature, K 298 328 358 378 Recheck k, s-1 1st attempt 3.46 x 10-5 1.5 x 10-3 3.34 x 10-2 0.21 Use the graphing tool above to make an appropriate plot and determine the activation energy, E, for this reaction in units of kilojoules_ X kJ/mol 4 Next) (1 of 1) Show Approach Select functions for the x-axis and the y-axis and create the plot that can be used to find the activation energy. The Arrhenius equatic Ea F/R (1) In k = In A - Inc y=b+mx
The first order reaction SO,CI, (g) --> SO2 (g) + Cl2 (g) has a rate constant of 2.90 X 10 s at a given temperature. Determine that concentration of SO,Cl, at 1,621 s if the initial concentration of SO,Cl, is 0.101 M.
Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant 1 03(g) O₂(g) + 0(g) k₁ 2 03(g) + O(g) → 20₂(g) k₂ Suppose also k₁ »k₂. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K2, and (if necessary) the rate constants k.1 and k-2 for the reverse of the two elementary reactions in the mechanism. = 0 k = 00 X 5 S ?
a The rate law for the reaction rogress 2NOBr(g) → 2NO(g) + Br2 (g) at some temperature is ΔΙΝΟΒ Rate = - = k[NOB1]² At If the half-life for this reaction is 2.00 s when [NOB1]o= 0.90 M, calculate the value of k for this reaction. k = L/mol·s Submit
Consider this reaction: 280; (g) → 2S0, (g) +0, (g) At a certain temperature it obeys this rate law. rate =(3.43 s")[so,] S SO Suppose a vessel contains SO, at a concentration of 0.590M. Calculate the concentration of SO, in the vessel 0.320 seconds later. You may assume no other 3 reaction is important. Round your answer to 2 significant digits. х10
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.)
A certain reaction has the following rate law: rate = k[X]³[Y]² Which of the following are the correct units for k? Select one: L³mol-3s-1 Ms-1 M³s O L?mol2s1 L5mol 5s1 Lmol-'s mol³L-3s-1 M's-1 L*mol-4s-1 mol?L-2s1
2 YO2 (g) + X2 (g) → 2 YO₂X (g) = -218 kJ/mol reaction AH rxn The reaction is first-order with respect to YO2 and first-order with respect to X₂. What is the relationship between the rate constant and activation energy of a chemical reaction?|
Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate = (8.98 × 10-4 ')[c,os] -1 S Suppose a vessel contains Cl₂05 at a concentration of 1.40M. Calculate the concentration of Cl₂O5 in the vessel 690. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Consider this reaction: 2C1,0, g) → 2C1, (6) + 50, (g) At a certain temperature it obeys this rate law. rate = (0.36 Ms)[C1,0,1 %3D Suppose a vessel contains Cl,0, at a concentration of 0.630 M. Calculate how long it takes for the concentration of Cl,0, to decrease to 5.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.
The decomposition of N»Os(g) to NO2(g) and O2(g) obeys first-order kinetics. Assuming the form of the rate law is: A[N,05] Rate = *[N,Os] At where k = 3.4 x 10-5 s-l at 25°C, what is the initial rate of reaction at 25°C where [N2O5]o = 4.1 x 10-2 M? а. 1.4x 10-6 mol/L's b. 3.4 x 10-5 mol/L's О с. 8.3 х 10-4 mol/L s d. 4.1 x 10-2 mol/L's e. none of these
The rate law for the reaction: NH4+ + NO₂ N₂ + 2H₂O is rate =k[NH4+][NO₂] It is found that the rate constant for this reaction is 3.05x10-4 M-1s-1. Calculate the rate of the reaction, including units, if [NH4*] is 0.265M and [NO₂] is 0.0803M. Attach File Browse Local Files