Nitrogen dioxide (NO₂) is an important pollutant in the troposphere. Nitrogen dioxide undergoes the following reaction:NO₂(g) NO(g) + 0(g)The rate constant of this reaction is 5.4×101 at 250 °C. At the boundary between the troposphere and stratosphere, where the temperature is abou-40.0 °C, the rate constant is reduced to 3.2x108.Note: Reference the Fundamental constants table for additional information.Part 1 of 2Calculate the activation energy for the decomposition of NO₂. Round your answer to 3 significant digits.kJmolPart 2 of 2What is the half-life of the reaction (in min) at 25.0 "C? Round your answer to 2 significant digits.minX

Given reaction:-NO2(g) NO (g)+ O(g)At 25 O C = 273+25 = 298 Kk1 = 5.4*10-3 s-1at -40 o C + 273 =…

Nitrogen dioxide (NO₂) is an important pollutant in the troposphere. Nitrogen dioxide undergoes the following reaction: NO₂(g) NO() +0(e) The rate constant of this reaction is 5.4×103 at 250 °C. At the boundary between the troposphere and stratosphere, where the temperature is about -40.0 °C, the rate constant is reduced to 3.2x10. Note: Reference the Fundamental constants table for additional information. Part 1 of 2 Calculate the activation energy for the decomposition of NO₂. Round your answer to 3 significant digits. kJ mol Part 2 of 2 X What is the half-life of the reaction (in min) at 250 °C? Round your answer to 2 significant digits. 0.8 min X

Nitrogen dioxide (NO₂) is an important pollutant in the troposphere. Nitrogen dioxide undergoes the following reaction: NO₂(g) NO() +0(e) The rate constant of this reaction is 5.4×103 at 250 °C. At the boundary between the troposphere and stratosphere, where the temperature is about -40.0 °C, the rate constant is reduced to 3.2x10. Note: Reference the Fundamental constants table for additional information. Part 1 of 2 Calculate the activation energy for the decomposition of NO₂. Round your answer to 3 significant digits. kJ mol Part 2 of 2 X What is the half-life of the reaction (in min) at 250 °C? Round your answer to 2 significant digits. 0.8 min X

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...

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Write the rate law for the decomposition of ammonium nitrite into nitrogen gas and water using the following data. NH4+1, Taq) + NO2(aq) → N2{g) + 2H2O) Trial [NH4*4]; [NO24}; Rate (M/s) 1 0.010 0.20 5.4x107 0.020 0.20 10.8x107 0.20 0.020 10.8x107 4 0.20 0.040 21.6x10-7 rate = 0.0027 M-1.5-1[NH4*+][NO21] rate = 0.000031s[NH4*1] rate = 0.0000012 s1[NH4*1] rate = 0.000029 s[NO21] O rate = 0.0000012 M-1.s1[NH4*1][NO24] O rate = 0.0000012 s1[NO24]
Ozone in the stratosphere can be depleted by the following reactions involving CI atoms: Step 1 (fast): CI + O3 <--> CIO + O2 Step 2 (slow): CIO + O -> CI + O2 (a) What is the rate law according to this mechanism? (b) Based on the rate law from part (b), what should be the units of the observed rate constant, k? Use time units of seconds.
given: 2O3 (g) --> 3O2 if the rate of O3 loss is 3.91 x10^-1 what is the rate of formation of O2
Potentially Useful Reference Information -Ea J R = 8.314 k = A· e RT mol ·K Complete the sentences below regarding the following reaction: CH4 + 2 O2 → CO2 + 2 H2O Methane (CH4) as water (H2O) The rate that oxygen (O2) is as the rate carbon dioxide (CO2) The possible answers are: appears, disappears, half as fast, twice as fast, or at the same rate.
The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCS) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1) CIO(g) + 0,(g) → Cl(g) + 20,(g) AH;xn = –122.8 kJ (2) 20,(g) → 30,(g) 0,(g)+Cl(g) → CIO(g) + 0,(g) AHn = -285.3 kJ (3) AĦxn = ? AHixn = kJ
For the gas phase decomposition of 1-chloropropane, CH;CH,CH,CH→CH;CH=CH, + HCI the rate constant in s- has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.77×104 K and a y-intercept of 31.0. The value of the rate constant for the gas phase decomposition of 1- chloropropane at 693 K is |s!. (Enter your answer to one significant figure.)
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The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCs) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1)ClO(g)+O3(g)⟶Cl(g)+2O2(g)ΔH∘rxn=−122.8 kJ(2)2O3(g)⟶3O2(g)ΔH∘rxn=−285.3 kJ(3)O3(g)+Cl(g)⟶ClO(g)+O2(g) ΔH∘rxn= ?(1)ClO(g)+O3(g)⟶Cl(g)+2O2(g)ΔHrxn°=−122.8 kJ(2)2O3(g)⟶3O2(g)ΔHrxn°=−285.3 kJ(3)O3(g)+Cl(g)⟶ClO(g)+O2(g) ΔHrxn°= ? ΔH∘rxn=ΔHrxn°=__________________________________________kJ
Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +03 (g) → NO3 (g) + O₂(g) 2 NO3 (g) + NO₂ (g) → N₂O5 (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. rate = k rate constant k₁ k₂ ロ→ロ X Ś
The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCs) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1)ClO(g)+O3(g)⟶Cl(g)+2O2(g)Δ?∘rxn=−122.8 kJ (2)2O3(g)⟶3O2(g)Δ?∘rxn=−285.3 kJ (3)O3(g)+Cl(g)⟶ClO(g)+O2(g) Δ?∘rxn= ?
Part B
2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for the reaction at 625 K.