**Study of Gas-Phase Oxidation of Nitrogen Monoxide**The reaction under investigation is:\[ 2NO(g) + O_2(g) \rightarrow 2NO_2(g) \]**Results Data Table:**| Experiment | Conc. NO (mol/L) | Conc. O₂ (mol/L) | Initial Rate (mol/(L·s)) ||------------|------------------|------------------|--------------------------|| Exp. 1 | 1.3 x 10⁻² | 6.7 x 10⁻² | 2.0 x 10⁻³ || Exp. 2 | 1.3 x 10⁻² | 0.13 | 3.9 x 10⁻³ || Exp. 3 | 2.6 x 10⁻² | 0.27 | 3.3 x 10⁻² || Exp. 4 | 0.95 | 8.7 x 10⁻³ | ? |---**Question: a**What is the experimental rate law for the reaction above?(Use $ k $ for the rate constant.)Rate law = \_\_\_\_[Submit Button]

For given Reaction , Let x be the order with respect to NO & y be the order with respect to O2…

This question has multiple parts. Work all the parts to get the most points. A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(9) + O2 (9) → NO2(9) Сonc. NO, molL Conc. Оz, тolL mitial Rate Exp. 1 1.3 x 10-2 6.7 × 10-2 2.0 x 10-3 mol/(L -s) Еxp. 2 1.3 x 10 2 0.13 3.9 x 10-3 mol/(L ·3) Еxp. 3 2.6 x 10 2 0.27 3.3 x 10-2 mol/(L-s) Exp. 4 0.95 8.7 x 10-8 ? a What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law = Submit

This question has multiple parts. Work all the parts to get the most points. A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the following results: 2NO(9) + O2 (9) → NO2(9) Сonc. NO, molL Conc. Оz, тolL mitial Rate Exp. 1 1.3 x 10-2 6.7 × 10-2 2.0 x 10-3 mol/(L -s) Еxp. 2 1.3 x 10 2 0.13 3.9 x 10-3 mol/(L ·3) Еxp. 3 2.6 x 10 2 0.27 3.3 x 10-2 mol/(L-s) Exp. 4 0.95 8.7 x 10-8 ? a What is the experimental rate law for the reaction above? (Use k for the rate constant.) Rate law = Submit

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

Related questions

Q: (Show or describe your work) Suppose the reaction A B has an equilibrium constant of Keq = [B]…

A: The overall rate for the forward reaction is the sum of forward reaction by the uncatalyzed pathway…

Q: 9. Calculate AH for the reaction C +H2O(g) → CÓ + H2 given the following data C+ O2→ CO2 2CO + 02 →…

A: Given data,

Q: A reaction, A +B+ C-> D, follows the rate law: Rate = k [A]2 [B]1 [cj0 What is the unit of the rate…

Q: 1a) The decomposition of ethanol at some constant temperature (above 500°C), over a copper surface,…

A: Solutions- 1a) The decomposition of ethanol at some constant temperature (above 500°C), over a…

Q: 6. Adsorption of hydrogen gas over palladium surface obey Freundlich's adsorption isotherm, as shown…

Q: E + PV E - PV -E + PV ΔΕ + Δ(PV) ΔΕ – Δ(PV) -ΔΕ – Δ(PV) RΤΔη -RΤΔη According to the definition of…

A: Enthalpy : Enthalpy is defined as the sum of internal energy of system and product of its pressure…

Q: Which of the following is not true? 1. When conditions are NOX-limited, the excess of VOCs in the…

A: We have asked to find out which statement is not true among the given four statements. The answer to…

Q: In a study of the rearrangement of cyclopropane to propene at 500 °C (CH₂)3 CH3CH=CH2 the…

A: Given:The reaction is:Graph of in s gives a straight line.The link between the rate of a chemical…

Q: Consider the gas-phase reaction to form hydrogen iodide, HI. The rate law has been determined…

A: If the rate law of any general reaction is given by : rate(r) = K [A]a [B]b It means the order of…

Q: A time-dependent pressure profile for the reversible reaction between A and B gases to produce C gas…

A: As A and B react reversibly to form C Balanced equation - A + B⇔C

Q: 34. A key step in the formation of sulfuric acid from dissolved SO, in acid precipitation is the…

A: Given that, the mechanism of formation of sulfuric acid from the dissolved SO2 in acid precipitation…

Q: CH3OH + TSOH OTs `OCH3

Q: For which of the following reactions would you predict AHxn° <0 and ASrxn° N2(g) + 3 H2(g) 2 NH3(g)

A: Change in enthalpy (∆H ): if ∆Hrxn < 0 indicates exothermic reaction and ∆Hrxn > 0…

Q: Industrially, nitric acid is produced by the Ostwald process, as represented by the following…

A: Answer:In this problem we have to convert the mass of HNO3 produced into mass of NH3 used by using…

Q: 20. The Haber-Bosch process, devised in the early 20th century, revolutionized global industry. It…

A: For general reaction, aA + bB → cC + dD Keq = [C]c[D]d/[A]a[B]b

Q: The gas phase decomposition of phosphine at 120 °C

A: Arrhenius equation tells how rate constant depends on the temperature which is its pre exponential…

Q: Analyze the following reaction mechanism: 1. Н.О, — Н,О +0 2. O+ CF,CI, –→ CIO + CF,CI 3. CIO + O, 2…

A: The steps involved in the given mechanism are, 1. H2O2 → H2O + O 2. O + CF2Cl2 → ClO + CF2Cl 3. ClO…

Q: A 0.213 M solution of HA has a pH of 2.87 at 25°C. What is the value of Ka for HA? (the answer…

Q: Determine the rate law and rate constant for the following reaction. Don't forget the units. Some of…

Q: A suggested mechanism for the gas phase decomposition of nitrous oxide is: step 1: Nz0 — Nz + 0 N₂O…

Q: Given the data in the image, what is the order of decomposition for NO2?

A: Given, We can determine the order of the reaction by plotting graphs of time versus concentration.…

Q: A study of the gas-phase oxidation of nitrogen monoxide at 25°C and 1.00 atm pressure gave the…

A: Chemical kinetics is the study of the reaction that how fast or slow a reaction is taking place. The…

Q: For the reaction 2 NO(g) + O 2 (g) → 2 NO2 (g) have the following data. Experiment 1 2 3: [NO], M…

A: Experiment [NO] (M)[O2] (M)Speed of consumption of NO (Ms-1)10.010 0.01020.0200.01030.0100.020

Q: Given the following results: Rate of Run Reaction [1] [H₂O₂] (M/s) 1.76 0.358 0.476 4.72 0.358 0.843…

Q: Determine the activation energy for the redox reaction Q2- + 2 R - Q* + 2 R". Rate…

A: Welcome to bartleby !

Q: b) The equilibrium constant Keq for the reduction of nickel (II) oxide, NiO, to nickel metal at754°C…

A: If reaction quotient is less than equilibrium constant then reaction will move forward If reaction…

Q: Which of the following statements is/are correct? (1) Catalysts are substances that increase the…

A: The given question is related to chemical kinetics and in the question, three statements are given…

Q: It may not surprise you to know that products can show up in the rate law. When the product(s)…

Question

100%

**Study of Gas-Phase Oxidation of Nitrogen Monoxide**

The reaction under investigation is:

\[ 2NO(g) + O_2(g) \rightarrow 2NO_2(g) \]

**Results Data Table:**

| Experiment | Conc. NO (mol/L) | Conc. O₂ (mol/L) | Initial Rate (mol/(L·s)) |
|------------|------------------|------------------|--------------------------|
| Exp. 1 | 1.3 x 10⁻² | 6.7 x 10⁻² | 2.0 x 10⁻³ |
| Exp. 2 | 1.3 x 10⁻² | 0.13 | 3.9 x 10⁻³ |
| Exp. 3 | 2.6 x 10⁻² | 0.27 | 3.3 x 10⁻² |
| Exp. 4 | 0.95 | 8.7 x 10⁻³ | ? |

---

**Question: a**

What is the experimental rate law for the reaction above?

(Use $ k $ for the rate constant.)

Rate law = \_\_\_\_

[Submit Button]

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

(7pts) The rate law for the reaction 3A C is Rate = 0.951 M' hr1 [A]? What is the half-life for the reaction if the initial concentration of A is 0.750 M? How long will it take for the concentration to be reduced to 0.050 M?
Consider the following gas phase reaction at constant volume: 2CH2N2(g) −→ 2N2(g) + C2H4(g) i) Given that the initial pressure is p0 calculate the total pressure after three quarters of the CH2N2(g) has reacted. ii) Derive an equation which shows how the total pressure varies as a function of the fraction, α, of the CH2N2(g) that has reacted. iii) Sketch a graph which shows how the pressure varies as a function of α
The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in acidsolutions is 2 Br– + H2O2 + 2 H+ → Br2 + 2 H2O ? = ?[H2O2][H+][Br−]If the concentration of H2O2 is increased by a factor of three, by what factor is the rate ofconsumption of Br– ions increased?
Expt. 1 2 3 NH; (aq) + NO; (aq) >Nz (aq) + 2 H2O (l) [NO₂] Rate (at 298 K) 0.020 M/s 0.020 M 0.020 M 0.030 M/s 0.010 M 0.0050 M/s [NH+] 0.010 M 0.015 M 0.010 M Determine the complete rate law (rate law and rate constant) for the reaction. Show all work. What is the initial rate of this reaction if the concentrations in Expt. 2 above are tripled. Show work. What is the rate of H₂O formation in Expt. 1? A 4th trial is conducted at 273 K, using the concentrations from Expt. 1. If the rate was found to be 0.016 M/s, calculate the activation energy of this reaction.
8. (15 marks) A reaction is written as A(g) At 298 K, k₁ =0.21 s.1. k.₁=5×10 Pa¹·s¹. B(g) + C(g). k-1 As the temperature increased from 298 K to 310 K, the values of k₁ and k., are doubled (denoted as k2 and K.2). (1) Calculate the rate constant k at 298K; (2) Calculate the activation energy of both forward and reverse reactions; (3) Calculate AH and AU for the reaction at 298K; (4) Calculate the reaction time at the whole pressure reaching to 152 kPa. The initial pressure of A(g) is 100 kPa and the reaction temperature is 298 K.
MN IN 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) + O,(g) → Cl(g) + 20,(g) AHxn = -122.8 kJ AHn = -285.3 kJ | rxn AHn = ? (3)°O + (3)OIƆ (3)1Ɔ+(3)*o (£) (3) 0E – (3)°07 (2) rxn %3D = UXHV kJ MacBook Pro Q Search or enter website name The & %23 $4 3. 4. 5. 7. 6. delete R H. K. re B. HE MOSISO command option
Consider the following elementary reaction: H,(9) +2NO(g) → N,0(g) +H,O(g) Suppose we let k, stand for the rate constant of this reaction, and k_, stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of H,O in terms of k, k_1, and the equilibrium concentrations of H, NO, and N,O. [H,0]= 0 %3D
Reaction CaCO3(s) Ca²+ (aq) + CO3²- (aq) AgCl(s) Ag+ (aq) + Cl(aq) AgBr(s) = Ag*(aq) + Br(aq) Agl(s) Ag+ (aq) + I¯(aq) Initial Concentrations ← [Ca²+] = 1.0 x 10-⁹ M [CO32] = 1.0 x 10⁹ M Ksp = [Ca²+][CO3²-1 X = 3.8 x 10-9 Initial Conditions Q = [1.0 × 10-⁹][1.0 × 10-⁹] = 1.0 x 10-18 Equilibrium Conditions [Ca2+] = 1.0 x 10⁹ M [CO32] 1.0 x 10.⁹ M Mass of CaCO3(s) = 0.0 g 42 of 7 What is the value of the reaction quotient, Q, which is calculated by substituting the actual initial values of [Ca²+] and [CO32] into the equilibrium expression?
Q:4-1 Consider the following reaction: 2 NO(g) + 2 H2(8) → N;(g) + 2 H,O(g) (a) The rate law for this reaction is first order in H, and second order in NO. Write the rate law. (b) If the rate constant for this reaction at 1000 K is 6.0 × 10ª M¯²s¯!, what is the re- action rate when [NO] = 0.035 M and [H,] = 0.015 M? (c) What is the reaction rate at 1000 K when the concentration of NO is increased to 0.10 M, while the concentration of H, is 0.010 M? (d) What is the reaction rate at 1000 K if [NO] is decreased to 0.010 M and [H,] is increased to 0.030 M? %3D Q:4-2 The iodide ion reacts with hypochlorite ion (the ac- tive ingredient in chlorine bleaches) in the following way: OCI- + I- –→ OI¯ + Cl¯. This rapid reaction gives the following rate data: [OCI¯] (M) [I-] (M) Initial Rate (M/s) 1.5 X 10-3 1.5 X 10¬3 1.36 X 10¬4 3.0 × 10–3 1.5 X 10–3 2.72 X 10¬4 1.5 × 10-3 3.0 × 10-3 2.72 X 10¬4 (a) Write the rate law for this reaction. (b) Calculate the rate constant with proper units. (c)…
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=69.0 kJ/mol. If the а - 1 rate constant of this reaction is 5.7 × 10² M - 1 S. at 304.0 °C, what will the rate constant be at 256.0 °C? Round your answer to 2 significant digits. - 1 - 1 k = || M •S x10 ?
3. The following reaction: A' (a) + B (ag + C (an)→ G* (ae) +2 H ) AH = -250 kJ There are two proposed mechanism: Mechanism 1 A' () + B aa) AB' a) + D (a) Step 1 AB" (a) (fast) + E (a) + Hm → G' sae) + H ) + D² (n) Step 2 (slow) Step 3 E (agi+ C (a) (fast) Mechanism 2: Step 1 AB' (a) A' (an) + B (ag) AB' (a) + C ja) (fast) Step 2 + G' (a) + 2 H() (slow) The reactions was determined to have the following rate law: r= k[A'][B] a) Which of the two proposed mechanisms is valid? Explain. b) List any reaction intermediates: catalysts: c) What is a rate determining step? d) If the activation energy for the overall forward reaction is 150 kJ, sketch the potential energy diagram for the above reaction; showing the overall reaction, the reaction mechanism, labelling the AHu, AHy, Eapu, Eag, reaction intermediates, and activated complex. rvs fwd drvs/
(5) IV. Hydrogen and carbon monoxide react to give formaldehyde under certain conditions. H2(g) + CO(g) = HCHO(g) The mechanism proposed for this reaction is H2(g) = 2 H(g) H(g) + CO(g) H(g),+ HCO(g) → HCHO What rate law is derived from this mechanism? Step 1 Step 2 Step 3 fast HCO(g) slow > fast