A chemistry graduate student is studying the rate of this reaction: 250; (2) – 2s0, (g)+O, (g) She fills a reaction vessel with So, and meas easures its concentration as the reaction proceeds: [so3] time (seconds) 0.0100 M 1.0 0.00627 M 2.0 0.00393 M 3.0 0.00247 M 4.0 0.00155 M Use this data to answer the following questions. Write the rate law for this reaction. rate 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.

A chemistry graduate student is studying the rate of this reaction: 250; (2) – 2s0, (g)+O, (g) She fills a reaction vessel with So, and meas easures its concentration as the reaction proceeds: [so3] time (seconds) 0.0100 M 1.0 0.00627 M 2.0 0.00393 M 3.0 0.00247 M 4.0 0.00155 M Use this data to answer the following questions. Write the rate law for this reaction. rate 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.

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

How much time does it take to reduce the concentration of NO2 by half by looking at the reaction process curve below?
At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N205(8)→ 4NO2 (g) + O2(g) When the rate of formation of O2 is 3.6 x 10-3 M/s, the rate of decomposition of N2O5 is. M/s. A) 0.00090 OB) 1.4 x 10-2 1.8 × 10-3 OD) 3.6 × 10-3 E) 4.4 x 10-4
A general reaction written as A + 2B → C + 2D is studied and yields the following data: [A]o [B]o Initial A[C]/At 8.00 x 10-3 mol/L·s 1.60 x 10-2 mol/L's 3.20 x 10-2 mol/L's 0.150 M 0.150 M 0.150 M 0.300 M 0.300 M 0.150 M What is the order of the reaction with respect to B? 0. 1 3 4 2.
NTERACTIVE EXAMPLE Reaction Rate Chloromethane reacts with iodide ion to yield iodomethane and chloride ion. CH;C1 +r- CH;I + CF A way to determine the rate of the reaction of chloromethane with iodide ion is to measure the disappearance of T from the solution. Suppose that the concentration of I was 0.21 mol IL at the start of the reaction. At the end of 20 min, the concentration dropped to 0.13 mol L. This difference is equal to a change in concentration of -0.08 mol IL. QUESTION What is the rate of reaction with respect to iodide ion? |× molIL'min
A chemistry graduate student is studying the rate of this reaction: 2HI (g) → H, (g) +I, (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time [HI] (minutes) 0.500M 1.0 0.241 M 2.0 0.159M 3.0 0.119 M 4.0 0.0946 M
A chemistry graduate student is studying the rate of this reaction: 2H₂PO4 (aq) → P₂O₂ (aq) + 3H₂O (aq) He fills a reaction vessel with H₂PO4 and measures its concentration as the reaction proceeds: time (seconds) [H₂PO4] 0 0.700M 10. 0.273 M 20. 0.170M 30. 0.123 M 40. 0.0967M Use this data to answer the following questions. Write the rate law for this reaction. x10 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. X rate = k k = 0 ?
Consider the following reaction: 2N₂O(g) → 2N2(g) + O2(g) Part A Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. Rate = 1 A[₂0] At O Rate = O Rate - Submit Rate = -A[₂0] At Correct Part B Rate = Submit A[N₂O] At Part C A[N₂0] At A[N₂O] At Previous Answers Submit Request Answer 1 A[N₂] 2 At At In the first 13.0 s of the reaction, 1.9x10-2 mol of O₂ is produced in a reaction vessel with a volume of 0.280 L. What is the average rate of the reaction over this time interval? Express your answer using two significant figures. IVE| ΑΣΦ Request Answer A[N₂] At 1 A[N₂] At 1/1 A[0₂] At A[0₂] At A[0₂] A[0₂] At Predict the rate of change in the concentration of N₂O over this time interval. In other words, what is A[N₂O]/At? Express your answer using two significant figures. IVE| ΑΣΦ ? M-s-1 ? M-s-1
A chemistry graduate student is studying the rate of this reaction: 2H, PO, (aq) → P,0, (aq)+ 3H,0 (aq) He fills a reaction vessel with H,PO, and measures Its concentration as the reaction proceeds: time [H, PO.] do (seconds) 0.400M 0.10 0.224M 0.20 0.156M 0.30 0.119 M 0.40 0.0967M Use this data to answer the following questions. Write the rate law for this reaction. rate = k M 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.
Use this data for the following four (4) questions: The relative initial rates of the reaction A2 + B2-products in vessels (a)-(d) are 1:1:4:4. The spheres represent the number of molecules of present at the beginning of the reaction. [Unshaded spheres = A2 molecules; shaded spheres = B2 molecules] %3D For example, vessel (a) contains 2 A2 molecules and 2 B2 at the beginning of the reaction. Rate = 1 Rate 1 Rate = 4 Rate = 4 %3D 2. 8. 80 (c) (a) 11) What is the order of reaction with respect to A2? (b) (d) BA 11) A))0 B) 1 C) 2 D) 3 12) What is the order of reaction with respect to B2? 12) C A) 0 B) 1 D) 3 13) o c 13) What is the overall order of reaction? A) 0 B) 1 D) B 14) 14) What is the rate law for this reaction? B) Rate k[B2]2 D) Rate = k[A2]2[B2]² A) Rate = k[A2]² %3D C) Rate = k[A2][B2] %3D %3D nation below: 15) 8. 8.
Cn.
over umme A chemistry graduate student is studying the rate of this reaction: 2N,0, (g) → 2N,0, (g) +O, (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds: time [N,0,] (seconds) 0.0500 M 1.0 0.0124 M 2.0 0.00710M 3.0 0.00497M 4.0 0.00382 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k Calculate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be X. sure your answer has the correct unit symbol.
The iodate ion reacts with sulfite ions in the reaction: 103 + 3SO3²1+ 3SO4². At what rate are the iodide and sulfate ions being produced if the sulfite ion is disappearing at a rate of 8.7 x 10.4 mol L ¹ s ¹? Rate of the iodide ion production is i Rate of the sulfate ion production is i Save for Later x 10-4 mol L ¹ s1. x 104 mol L-¹ s-1. Attempts: 0 of 10 used Submit Answer