[S208 2-J, M [S203 2-J, M 0.08000 8.0*10-4 0.04000 8.0*10-4 0.02000 8.0*10-4 0.04000 8.0*10-4 0.04000 8.0*10-4 Runs [H, M Reaction time,s Rate, M/s 1 0.02000 49.10 2a 0.02000 106.10 0.02000 197.44 69.20 53.05 4 0.03000 0.04000
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- Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?Reaction Conc. Na2S203 Conc. HCI Δ Abs. A Time (s) Rate (Δ Abs./Δ Time) 1 0.10 M .30 M 1.3686611 1.007568 1.358380874 2 0.10 M .15 M 1.5360817 0.300349 5.114311671 3 0.050 M .30 M 1.2267196 0.01870913 65.56796601 4 0.025 M .30 M 0.9563164 0.02870913 11.3085840 POSTLAB QUESTIONS 2. Compare the rates of reactions 1 and 2. What is effect on the reaction rate of halving the acid concentration? What is the order of the reaction in hydrochloric acid?B. Concentration Table B: Reaction Rate of Na S O/HCI Beaker # 12345 A-Volume- of 0.15 M Na,S,O, (aq) used / ml. 50.0 40.0 30.0 20.0 10.0 B- Volume of water/mL. 0.0 10.0 20.0 30.0 40.0 Total volume (A+B) /ml 50.0 50,0 50.0 50.0 50.0 *Concentratio n of Na,8,0, (aq) /mol L 15 .12 090 060 030 Plot two graphs: 1. Time vs concentration of Na.S,O, (aq) 2. 1/Time vs concentration of Na S.O, (aq) Time/s 22.5 27.3 35.1 60.0 159.1 Explain the observations (relationship between concentration and time). 1/time/ 0444 0366 *Use civic₂V; to determine the concentration of the diluted sodium thiosulphate solution (beakers 2-5). On how to use this dilution formula, then, please watch: 0285 0167 00629
- Use the data in the table below to answer the following questions. Reaction : 4.0 M Acetone (in mL) 1.0 M HCl (in mL) 0.005 M Iodine (in mL) H2O (in mL) Time - 1st Run Time - 2nd Run Avg. Rxn. Time Temp (°C) 1 8 8 8 26 23 2 4 8 8 30 23 3 8 4 8 30 23 4 8 8 4 30 23 Which two experiments should be compared to determine the exponent in the rate law for acetone? Which two experiments should be compared to determine the exponent in the rate law for HCl? Which two experiments should be compared to determine the exponent in the rate law for iodine?1: Consider: H₂(g) + 12 (g) = 2 HI (g). The [1₂] and [HI] are plotted against time. Please compute A[1₂]/AT and A[HI]/AT. Hint: the slope of the [HI] versus time graph is A[HI]/AT Concentration (M) 1.4 1.2 1 0.8 0.6 0.4 0.2 0 0 Concentrations at different times 5 10 15 ●● 20 Elapsed time (s) 25 [12] [HI] 30 35 40For the exothermic reaction 4 NH3(g) +7 02(g)- => 4 NO2(g) + 6 H20(g) which change will increase the quantity of NO2 in the mixture? O A. increasing temperature OB. decreasing container volume OC. adding Ne(g) O D. adding H20(g) O E. adding a catalyst
- Answer the following question using the reaction coordinate diagram shown below. 280+ 240+ 200 160 120- 80 40 Time Which of the following best describes the forward reaction? A. Neither exothermic nor endothermic B. Endothermic C. Exothermic Heat content (H) kilojoulesConsider the data from the previous question again. A-> B rate= 4.0 M/S B-->C rate = 1.5 M/min C-->D rate = 6.5 M/hour In the overall reaction A--> D, which step determines how fast the product D is made? a. A-->D Ob. A-->B O C. B-->C Od. C-->DAnswer the following question using the reaction coordináte diagram shown below. 280- 240- E200- 160- 120- 80 + 40 Time Which of the following best describes the reverse reaction? A. Exothermic B. Endothermic C. Neither exothermic nor endothermic bp 96 Heat content (H) kilojoules
- The diagram below shows the energy profile for a reaction. D M. В E C A Reaction progress Species labeled D is called EnergyReaction 1 Reaction Progress 6. A(g) + B (g) →C(g) For the reaction above AH=+100 KJ. The forward reaction starts slowly but speeds up when a catalyst is added. Below write out a potential energy diagram for the reaction. Be sure to label the following on your diagram: a. Both axes b. Product and reactant energy c. Activated complex energy d. Sketch the curve e. Activation energy f. Enthalpy10. The rate law of the overall reaction is k[A][B]0. Which of the following will not increase the rate of the reaction? A. increasing the concentration of reactant AB. increasing the concentration of reactant B C. increasing the temperature of the reaction D. adding a catalyst for the reaction 11. Which of the following would NOT increase the rate of reaction? A. raising the temperature B. adding catalyst C. increasing the volume of the container D. increasing the concentration of the reactants 12. What is the correct expression of the rate of a chemical reaction? A. grams per mole B. energy consumed per mole C. molarity per second D. volume of gas per unit time 13. Why an increase in temperature increases a reaction rate? A. only because there are more collisions B. only because the particles collide with greater energy C. by providing an alternative pathway for the reaction to follow D. because the particles collide more frequently and with greater energy 14. Which condition…