A chemical engineer is studying the rate of this reaction. 2SO 3 (g). → 2SO2 (g) + 0, (g) She fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds. Here's a graph of her data: 0.8- 0.6- 0.4 0.2- 0.8 1.2 0.2 0.4 0.6 t (seconds) TO (w) [*os] Use this graph to answer the following questions: What is the half life of the reaction? ||s 4/2 = 0s Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in Calculate the value of the rate constant k. SO 3: k = Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of SO, in the engineer's reaction 3 vessel after 2.40 seconds have passed. [so,]= OM Assume no other reaction is important, and continue to assume the rate is first order in SO 2. Round your answer to 2 significant digits.

A chemical engineer is studying the rate of this reaction. 2SO 3 (g). → 2SO2 (g) + 0, (g) She fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds. Here's a graph of her data: 0.8- 0.6- 0.4 0.2- 0.8 1.2 0.2 0.4 0.6 t (seconds) TO (w) [*os] Use this graph to answer the following questions: What is the half life of the reaction? ||s 4/2 = 0s Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in Calculate the value of the rate constant k. SO 3: k = Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of SO, in the engineer's reaction 3 vessel after 2.40 seconds have passed. [so,]= OM Assume no other reaction is important, and continue to assume the rate is first order in SO 2. Round your answer to 2 significant digits.

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

Using the data in the table, determine the rate constant of the Trial [A] (M) [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.200 0.400 0.0155 2 0.200 0.800 0.0155 A + 2B » C+ D 3 0.400 0.400 0.0620 Units k =
Hydrogen iodide decomposes slowly to H2 and 12 at 600 K. The reaction is second order in HI and the rate constant is 9.7 × 10-6 M-1 s-1. Part A What is the half-life (in days) of this reaction when the initial HI concentration is 0.100 M? Express your answer using two significant figures. ΕΠΙ ΑΣΦ t 1/2 = Submit Request Answer 0 ? days
The reactant concentration in a zero-order reaction was 0.100 M after 100 s and 4.00×10-2 M after 400 s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash.
Consider the schematic reaction A → P. If the reaction is ½ order with respect to A then the integrated rate law is [A]½ = –kt/2 +[A]0½ a) What plot would you construct to determine the rate constant k for the reaction? b) Derive the half-life for this reaction? Will it depend on initial concentration of the reactant?
The reaction 2A – 3B obeys the rate law R = k [A] with a half-life of 3.25 s. How much B(in M) will be produced in 12.8 s if you start with 0.248 M of A? Express your answer in decimal notaion rounded to three significant figures. Type your answer.
-1 -1 At a certain temperature the rate of this reaction is second order in HI with a rate constant of 1.0M S 2HI (g) → H₂(g) + 1₂ (g) Suppose a vessel contains HI at a concentration of 1.33M. Calculate the concentration of HI in the vessel 7.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś ?
Note: This is a The reaction below is first order with respect to NO and second order with respect Cl, Determine the value of the rate constant and write the rate law. 2 NO (2) + Cl2 (g) 2 NOC1 (g) Initial [Cl2] Initial Rate (M/s) Experiment Initial [NO] 0.0125 M- 0.0255 2.27 x 10- 1 0.0125 M 0.0510 9.08 x 10-5 3. 0.0250 M 0.0255 4.55 x 10-5 Rate = 0.00370 M-2s [NO2el [Cl@] Rate = 2.79 M2s [NO2 [Cl(g)] ORate= 0.0712 M-'s [NO] [Clgl* Rate = 5.70 Ms [NOl' [Clze1 Rate = 5.70 M2s [NOl [Cl@l' 2,41 [Cl(e) Rate = 2.79 Ms" [NOe)l' [Cle भजको को तो Rate = 0.00370 M²s [NO2l [Cl2el Rate = 0.0712 M's [NO2] [Cl]
The generic reaction shown below follows second-order kinetics. 3 A + 2 B → products The half-life of A is 65.0 seconds when the initial concentration of A is 0.858 M. Determine the value of the rate constant for this reaction. Round your answer to 3 significant figures. You do not need to enter a unit.
If a reaction involving a single reactant is first order with a rate conatsnt of 4.50 x 10^-2 s^-1, how much time is required for 53% of the initial quantity of reactant to be used up?
What is the half-life for a particular reaction if the rate law is rate = (1211 M*min⁻¹)[A]⁰ and the initial concentration of A is 0.250 M?
For the given generic reaction, the concentration of A and the amount of time that is required to decrease the concentration to one-half of the initial concentration, t1/2, are directly proportional. Therefore, a decrease in the concentration of A shows a proportional decrease in the half-life, t1/2.
For the reaction A → B, a plot of ln[A] vs. time yields a straight line with the equation y= -0.423 + 0.092x. What is the reaction order with respect to A? What is the half-life of the reaction in (s) ? What was the initial concentration of A (M) ?