The reaction 2 NO(g) + O2(g)-> 2 NO2(g) is important in forming smog. Undercertain conditions, the rate law for a the reaction israte = 4.0 x 103 1/M2*s * [NO]2* [O2]What is the rate when [NO]=0.020 M and [02]=0.035 M?Oa.5.6 x 108 M/s.Ob. 9.8 x 10-2 M/SOc. 9.8 x 10-8 M/s What is the rate when [NO]=0.020 M and [O2]=0.035 M?Oa.5.6 x 10-8M/s.Ob.9.8 x 10-2 M/sOcC.9.8 x 10-8 M/sOd.9.8 x 10-5 M/sle.5.6 x 10-2 M/s

Rate of a chemical reaction is defined as the speed with which the reaction proceeds. It determines…

The reaction 2 NO(g) + O2(g) -> 2 NO2(g) is important in forming smog. Under certain conditions, the rate law for a the reaction is rate = 4.0 x 10-3 1/M2*s * [NO]2* [O2] What is the rate when [NO]=0.020 M and [021=0.035 M? Oa. 5.6 x 10-8 M/s. Ob. 9.8 x 10-2 M/s Oc. 9.8 x 10-8 M/s

The reaction 2 NO(g) + O2(g) -> 2 NO2(g) is important in forming smog. Under certain conditions, the rate law for a the reaction is rate = 4.0 x 10-3 1/M2s [NO]2* [O2] What is the rate when [NO]=0.020 M and [021=0.035 M? Oa. 5.6 x 10-8 M/s. Ob. 9.8 x 10-2 M/s Oc. 9.8 x 10-8 M/s

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: 2 NO2(g) + F(g) → 2 NO,F(8) is plausible. The rate law is rate = k[NO2] [F2]

A: Order of the reaction is second reaction mechanism is define so that we can calculate intermediate…

Q: The decomposition reaction of N½O5 in carbon tetrachloride is 2N½O5 --> 4NO2 + O2. The rate law is…

A: The reaction given is

Q: Initial rate data is given in the table for the following reaction. 2 NO(g) + O₂(g) - 2 NO₂(g) What…

A: The sum of the exponent terms in the rate law for a chemical reaction is known as the order of the…

Q: Consider the reaction: A(B0)3 → AO + BO2. Which of the following is a possible rate law for the…

A: Rate law: It is the rate law of a reaction that relates the concentration of each reactant to the…

Q: Asses.1: The initial-rate data in the table below were obtained for the represented reaction. A+B 2C…

Q: Given the following balanced equation, determine the expression for the rate of reaction with…

A: The rate of the chemical reaction depends solely on the initial concentration. The rate is equal to…

Q: A chemical engineer is studying the rate of this reaction. 2NH3(g) = N2(g) + 3H2(g) He fills a…

A: The half-life (t1/2) is the time required to reduce one half of its initial concentration.The…

Q: 2NO2 → 2NO + O2 obeys the rate law: Rate = 1.40 x 10–2 M-1 s-1[NO2]2 at 500° K. If the initial…

Q: 2N2O5 (aq) → 4NO₂ (aq) + O₂(g) In a previous step, you calculated the rate of disappearance of N2O5…

Q: You perform some experiments for the reaction A -------> B + C and…

A: Given Reaction A → B + C (a) If A is tripled then rate increases by a factor 81 Rate…

Q: Consider a reaction governed by the following rate law: Rate = 0.38 M-1 s-1⌈A⌉2 How long does it…

A: Recall the data, Rate law, Rate=0.38 M-1 s-1 [A]2 power of A is 2, therefore order of reaction=2 At…

Q: Consider the reaction described by the equation C,H,Br, (aq) + 3I-(aq) C,H,(g) + 2 Br (aq) + I, (aq)…

Q: Ozone decomposes to oxygen according to the equation 2 O3(9) - 3 02(9). Write the equation that…

Q: Dinitrogen pentoxide decomposes according to the reaction 2N2O5 (g) → 4NO2 (9) + O2(9) At 45°C the…

A: Rate determining step is a step which is the slowest step of the reaction and the reactant involving…

Q: A reactant decomposes with a half-life of 155 s when its initial concentration is 0.271 M. When the…

A: We have to predict the order , rate constant and unit .

Q: For the reaction A + BC the rate law is: rate = k[B]2. Which plot will yield a straight line? FD1

Q: Initial Concentration (mol/L) Rate of Appearance of C A В (mol/L.s) 0.10 0.10 2.0 x 103 0.20 0.10…

A: We know that :- Rate = K [ A ]x [ B ]y Where, x is Order of A and y is order of B

Q: 7. Substances P and Q react together to form products and the overall order of the reaction is…

A: Rate equation may be defined as an equation that links the rate of forward reaction with the…

Q: Overall: 2X₂ (g) +Y₂(g) → 2X₂Y (g) Step 1: 2X₂(g) → 4X (g) (slow) Step 2: 4X (g) + Y₂(g) → 2X₂Y (g)…

Q: For this A + B → P, and the order of reaction with respect to A is first order and with respect to…

Q: Consider this reaction: H₂CO3 (aq) → H₂O (aq) + CO₂ (aq) At a certain temperature it obeys this rate…

A: Given,The reaction:

Q: 1.) Consider the reaction below at 100°C T2U (g) → 2 T (g) +U (g) When [T2U] = 0.250 M, the reaction…

Q: on 2 NO(g) + Cl2(g) --> 2 NOCI(g) given the following mechanism 1. NO(g) + Cl2(g) = NOCI2(g) 2.…

A: Rate law of reaction can be written by using rate determining step , so first need to identify rate…

Q: С,Н, Вr, (aq) + 3Г(аq) — C,H,(g) + 2 Br¯(aq) + I5 (aq) ne rate law is k[C,H¸B1, ][I¯] rate = nere k…

Q: The reaction below has a rate constant of 2.6 x 10-3 L²mol-2.s-¹. If the rate of disappearance of O₂…

A: The speed of the chemical reaction is measured in terms of the rate of the reaction.rate of the…

Q: The reaction 2A + 3B+H*--> products was studied. The rate law for this reaction was reported to be…

A: The reaction involved is 2A + 3B + H+ ----> Products. Rate law is Rate = k[A]2[B]2[H+] The orders…

Q: For the reaction : NO2CI(g) + NO(g) rate equation is first order in NO. What is the rate constant,…

A: Given: A = 8.3× 108 Ea = 28.9 kJ/mol

Q: The following data was collected for the reaction 2 Mg + O2 --> 2MgO Determine the order for…

A: The rate of the reaction expresses how fast the reaction is occurring and is expressed in terms of…

Q: Given the data and the reaction below, write the rate law including the value of the rate constant,…

A: A constant quantity useful in deriving rate law and relating the reactants' concentration with…

Q: The mechanism for NO2 (g) + CO (g) → NO (g) + CO2 (g) is thought to be: 2 NO2 → NO3 + NO (slow) NO3…

A: Given :- NO2(g) + CO(g) → NO(g) + CO2(g) Mechanism :- 2NO2 → NO3 + NO (slow) NO3 +…

Q: If the reaction 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) is first order in H2 and first order in…

A: Order of a reaction is the sum of stoichiometric coefficients which are present in the power of the…

Q: Bromide ion is oxidized by bromate ion in acidic solution. 5Br (aq) + BrO3 (aq)+ 6H"(aq)→ 3Br2(aq) +…

A: Order of a reaction: Sum of the power of concentration terms of all the reactant species in the rate…

Q: Hydrogen iodide decomposes when heated, forming H2(g) and I2(g). The rate law for this reaction is…

Q: For a reaction that follows the general rate law, Rate = k[A][B]?, what will happen to the rate of…

A: Given , Rate = K [A] [B]2 Now, we consider initially ,[A] = X and [B] = X And The concentration of…

Q: Consider this reaction: 2N,0, (g) → 2N,0, (3) + O, (g) At a certain temperature it obeys this rate…

Q: A hypothetical gas phase reaction is shown as: X2Y2(g) + 2Y2(g) → X2Y6(g). The rate law is given as:…

Q: A student ran several experiments for this reaction: 5 CH3COOH(aq) + 8 MnO4 (aq) + 24 H*(aq) → 8 Mn2…

Q: 5. The reaction H2 (g) + 12 (g) → 2 HI (g) has the following mechanism proposed: Fast 12 (g) = 21…

Q: The reaction shown below has the rate law rate=k[NO]2[Cl]. Determine the overall reaction…

A: To solve this problem we have to determine the overall reaction order of the given reaction. For the…

Q: The rate of a certain reaction is given by the following rate law: rate=k[H₂][1₂] Use this…

A: The rate expression for a certain reaction given is ,rate = k[H2][I2]Rate law Rate law gives the…

Q: What is the rate law of the reaction below: NO (g) + NO (g) -> N2O2 (g) fast N202(g) + O2(g) -> 2NO2…

A: Rate of reaction is defined as the speed with which reactants are converted into products. It…

Q: The scenes below show two experiments at a given temperature and volume involving reactants X…

A: We have to observe the given figure very carefully. From the rate law, we will get enough…

Question

The reaction 2 NO(g) + O2(g)
-> 2 NO2(g) is important in forming smog. Under
certain conditions, the rate law for a the reaction is
rate = 4.0 x 103 1/M2*s * [NO]2* [O2]
What is the rate when [NO]=0.020 M and [02]=0.035 M?
Oa.
5.6 x 108 M/s.
Ob. 9.8 x 10-2 M/S
Oc. 9.8 x 10-8 M/s

What is the rate when [NO]=0.020 M and [O2]=0.035 M?
Oa.
5.6 x 10-8
M/s.
Ob.
9.8 x 10-2 M/s
Oc
C.
9.8 x 10-8 M/s
Od.
9.8 x 10-5 M/s
le.
5.6 x 10-2 M/s

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

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

A certain reaction has a rate law of R=k[AJ<[B] with a rate con- stant equal to 4068.27 M?s². The rate of reaction when [A] is .025 M and [B] is 0.30 M is .7628 M/s. What is the rate of reaction when [A] is equal to 0.001 M? a. 1.22x10³ M/s b. 1.22 M/s c. 0.366 M/s d. 2.28x107 M/s
Consider the following chemical equation: Overall Reaction: A B2 + BC - AB + C + B2 The proposed mechanism is as follows: BC – B+ C (slow) A B2 + B = AB+ B2 (fast) What is the rate law? Rate = k[B C] O Rate = k[A B,][B] Rate = k[C] O Rate = k[B][C] Rate k[A B2][B C) Rate = k[A B][B,] Rate = k(A B2]
Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate =(0.0913 s¯¹)[C₁₂05] Suppose a vessel contains Cl₂05 at a concentration of 0.460M. Calculate the concentration of C1₂O5 in the vessel 9.70 seconds later. You may assume no other reaction is important. 25 2 Round your answer to 2 significant digits. [ M x10
Consider the reaction below at 100oC T2U (g) ⟶⟶ 2 T (g) + U (g) When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, A. Which is the rate law of this reaction? B. which is the numerical value of the specific-rate constant, k, for this reaction? C. Which are the units for the specific rate constant, K? D. At whic rate is T generaten when [T2U] is 0. 111 M? E. if given an initial reactant concentration [T2U]o = 0.250 M, what is [T] after 15 minutes have elapsed?
Hi I need help with the last 2 questions
8 OKONETICS AND EQUILIBRIUM Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2N₂O, (g) → 2N₂O, (g) + O₂(g) He fills a reaction vessel with N₂O, and measures its concentration as the reaction proceeds: time (minutes) 0 10. [N₂O,] Explanation 0.300M 0.121 M 20. 0.0762 M 30. 0.0555 M 40. 0.0436M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. Check rate & D www-awa.aleks.com k= D.D X
The following reaction has rate law r = k[C4H6] 2 , where k = 0.014 M-1 s -1 What is the concentration of C4H6 (in M) after 3.0 hours, if [C4H6]o = 0.025 M? A. 0.0052 M B. 0.024 M C. 0.012 M D. 0.0060 M
16 redone
The initial concentration was 3.0 M and the rate law is shown below. What is the concentration of T after 25.0 minutes? Rate = 2.1 x 10-² M. s-¹ [T] = [?] M [T], M Enter
The following data was collected for the reaction 2 Mg + O2 --> 2MgO Determine the order for each reactant and write the rate law. Trial [Mg] (mol/L) [O2] (mol/L) Measured Rate(M/s) 1 .10 .10 2.0x10-3 2 .20 .10 4.0x10-3 3 .10 .20 8.0x10-3 According to this data the order for Mg is Answer (enter a number).
The data in the table below were obtained for the reaction: 2A + 2B — зс Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.775 0.321 0.082 2 1.51 0.321 0.082 3 0.775 0.963 0.738 The rate law for this reaction is rate = O A. k[A][B]² B. k[B]2 c. k[A][B] O D. K[A]2{B] O E. K[A]²[B]2
The rate of reaction NO2(g)+ CO(g) ----> NO (g) + CO2(g) was determined in three experiments at 225 C. The results are given in the following table: a. Determine the rate law for the reaction. Calculates the value of the rate constant at 225 C. Calculate the rate of appearance of CO2 when [NO2]=[CO]= 0.527