4) You want to determine the rate law of the reaction below. A B C+D You run the reaction three times and monitor the product C using spectroscopy. You are then able to calculate the initial rates of each reaction simply by taking the slope of the concentration of C vs time. Here is the data. Initial Rate 1.0 x 10 M/s 4.0 x 101 1.6 x 10 Exp LA 0.40 M [B] 0.30 M 0.80 0.80 0.30 3 0.60 What is the order with respect to A? What is the order with respect to B? What is the rate law? What is the value of the rate constant? General form for rate law is rate = k (reactant 1]"[reactant 2]^[reactant 3]'..

4) You want to determine the rate law of the reaction below. A B C+D You run the reaction three times and monitor the product C using spectroscopy. You are then able to calculate the initial rates of each reaction simply by taking the slope of the concentration of C vs time. Here is the data. Initial Rate 1.0 x 10 M/s 4.0 x 101 1.6 x 10 Exp LA 0.40 M [B] 0.30 M 0.80 0.80 0.30 3 0.60 What is the order with respect to A? What is the order with respect to B? What is the rate law? What is the value of the rate constant? General form for rate law is rate = k (reactant 1]"[reactant 2]^[reactant 3]'..

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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6. The phosphorus content in a 0.3004-g sample was precipitated as (NH4);PO4 .12M0O3 a slightly soluble precipitate. The precipitate was filtered, washed, and further redissolved in acid. The resulting solution was treated with an excess of Pb²* resulting in the formation of 0.3017 g of PbMoO4. Calculate the % w/w of P2Os.||
A (aq) + ...B(aq) C(s) + D (aq) ... .. Experimental | Volume of B/ mL Mass of Run precipitate/g 1 1.2 5.40 2 1.4 7.24 1.6 9.02 4 1.8 9.90 2.0 10.86 6. 2.2 10.90 7 2.4 10.88 8 2.6 10.84 9. 2.8 10.86 A series of experiment was performed to determine the mole ratio of a given reaction. 1 mL of 1 Molar A added to nine beakers, then the increasing amount of 1 Molar B added to these beakers. Volume of B and mass of precipitate of C are given in the table below. Find the mole ratios through plotting a graph.
pl2) please answer and explain. If the 125 mL Erlenmeyer flasks used in this experiment, (Standardization of a Sodium Hydroxide Solution), were washed and rinsed with distilled water but not dried prior to use, how owuld this affect the calculatoed concentration of the standardized NaOH solution?
N-mh9Q_Lby/o81Y1_cekwly?1oBw7QYjlbavb International Stude.. A Checkout Shippin.. Seedlang | Start Sp... Classic Rock 80's -. C Courses at Kutztow.. Pennsylvania Acces. * Department of Hu.. O CHEMICAL REACTIONS Solving for a reactant using a chemical equation Ammonium perchlorate (NH,Clo,) is the solid rocket fuel used by the U.S. Space Shuttle. It reacts with itself to produce nitrogen gas (N,), chlorine gas (Cl,), oxygen gas (O,), water (H,O), and a great deal of energy. What mass of nitrogen gas is produced by the reaction of 5.43 g of ammonium perchlorate? Round your answer to 3 significant digits. II
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Answer in not more than 5 sentences per question 1. Discuss the a) direct method of weighing b) indirect weighing using the analytical balance. 2. Explain how suction filtration is carried out in the laboratory. Give the important points that must be observed in doing the process. 3. Explain why it is important to wash the precipitate. Can distilled water be used to wash all types of precipitates? 4. Discuss how to use a desiccator. When should a desiccant be replaced? Give 2 examples of substances used as desiccants.