2. 4. 6. 8. =10 A chemical engineer is studying the rate of this reaction. 2NH, (g)→ N, (g) + 3H, (g) He fills a reaction vessel with NH, and measures its concentration as the reaction proceeds. Here's a graph of his data: 0.20 0.15 0.10 0.05- 0.2 0.4 0.6 0.8 1.2 t (seconds) Continue 2020 McGraw Hill Education. All Rights Rese 16 ARR tv MARook Air (w)[°HN] Use this graph to answer the following questions: What is the half life of the reaction? %3D x10 Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in NH2. Calculate the value of the rate constant k. k = 0 Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of NH, in the engineer's reaction vessel after 2.10 seconds have passed. [NH,] = 0M %3D Assume no other reaction is important, and continue to assume the rate is first order in NH2. Round your answer to 2 significant digits. Continue O2020 16 APR.

2. 4. 6. 8. =10 A chemical engineer is studying the rate of this reaction. 2NH, (g)→ N, (g) + 3H, (g) He fills a reaction vessel with NH, and measures its concentration as the reaction proceeds. Here's a graph of his data: 0.20 0.15 0.10 0.05- 0.2 0.4 0.6 0.8 1.2 t (seconds) Continue 2020 McGraw Hill Education. All Rights Rese 16 ARR tv MARook Air (w)[°HN] Use this graph to answer the following questions: What is the half life of the reaction? %3D x10 Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in NH2. Calculate the value of the rate constant k. k = 0 Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of NH, in the engineer's reaction vessel after 2.10 seconds have passed. [NH,] = 0M %3D Assume no other reaction is important, and continue to assume the rate is first order in NH2. Round your answer to 2 significant digits. Continue O2020 16 APR.

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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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.
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The reactant concentration in a zero-order reaction was 8.00×10−2 M after 150 s and 3.50×10−2 M after 395 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.
A chemical engineer is studying the rate of this reaction. 2N,0, (g) → 2N,O4g)+O2 (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds. Here's a graph of his data: 2 1.5 - 0.5 0. 0.2 0.4 0.6 0.8 1.2 t (s) (x) [°o°n]
The rate of a certain reaction was studied at various temperatures. The table shows temperature (?) and rate constant (?) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, ?a , for this reaction? What is the value of the pre‑exponential factor (sometimes called the frequency factor), ? , for this reaction? Temperature (K) k (s^-1) 400 0.0000173 580 7.43
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8. C4H8(g) 2C₂H₂(g) Determine the order of the reaction and the rate con- stant based on the following pressures, which were recorded when the reaction was carried out at 430°C in a constant-volume vessel. Time (s) 0 2,000 4,000 6,000 8,000 10,000 PC,H, (mmHg) 400 316 248 196 155 122 M
The rate constant for the second order reaction 2 NO2 - 2 NO + O2 is 0.24 M's. If a 1.38 M sample of NO2 reacts for 47.7 seconds, what concentration of NO2 wil remain? Report your answer to two decimal places. |Al = - kt +|Alo InJAl = - kt + InlAlo TAI = kt + TAlo
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0017 M.s¹: Suppose a 300. mL flask is charged under these conditions with 450. mmol of hydrogen iodide. How much is left 200. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 2 HI (9) H2(g)+1₂(g) B = X x10
The reactant concentration in a first-order reaction was 5.80×10−2 M after 40.0 s and 1.60×10−3 M after 70.0 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.