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CHEM 281 Study Guide - Final Guide: Carran, List Of Virtual Boy Games, Scantron Corporation

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orangecicada704

19 Jul 2018

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Queen's University

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Please answer all multiple choice questions on a separate scantron sheet provided (do not use the virtual lab scantron sheet) Answer all questions, no marks are deducted for wrong answers. Please answer all short answer questions clearly in the answer booklet provided. Total pages 15 including this page and periodic table. Proctors are not able to answer questions on course content. You may use the back of this exam booklet as scrap paper. Molecular models are allowed in the exam contained in a clear ziplock bag. I: i and ii, iii and iv, v, ii, i and v. Iv: i and ii, ii and iii, iii and iv, i and iv, ii and iv. Iv: i, ii, iii, i, ii, iii, i, iv, v. Use separate scantron sheet and answer booklet provided: which compound listed below is a secondary alcohol, ch3chch2ch3.

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Show transcribed image text correctly.Completion and turning in of the entire review will result in an additional +3 pts on your final exam. Show all work to get extra credit. Please contact your instructor for clarification or specific questions. Report the following answers to the following problems with the correct number of significant figures and units: 1. 1 (0521 g 0.4953 0098 61â-24.135ë¯¸+1(120 64 g 4.1847 a)(21st-241530 1 (98.61 C-24.135)120.64g 4.1 21.5Â°C-24.153C) 0.0213548 moles b. (00020334-ern) + ((61210 goles Og) 0.002030 moles 1.02 moles (68.79 mlt29.901 ml) (26.3-0.230) c. 2. You are drying a sample of Bas(POsh. After 5 minutes of drying it weighs 1.2034 g. You continue to dry the sample for another 5 minutes and it now weighs 1.9346 g. What is the percent change in mass? 3. What is the percent mass of carbon in sodium carbonate? 4. What is the density of water at 23.1051Â°c? Use Table 1.1 on page 27 of your lab manual to help. 5. Based on the following reacts, predict the products. Write the balanced molecular equation, total ionic equation, and net ionic equation. All reactions are done in water a. Sodium chloride +silver (I) nitrate b. Calcium bromide + iron (III) sulfate c. Ammonium phosphate+ nickel (II) nitrate d. Hydrochloric acid+ calcium carbonate 6. Write the two balanced chemical reactions for a. Copper (II) oxide reacting with methane under high heat b. Copper (1) oxide reacting with methane under high heat 7. You analyze a mixed sample of copper (1) oxide and copper (II) oxide. The plot and trendline for mass of copper versus mass of mixture yields a slope of 0.8031. What are the mass percents of copper (0) oxide and copper (II) oxide in the mixture?
8. During week 1 of the Empirical Formula Lab you extinguished your "L-tube" flame without waiting 9. 20.00 ml of a 0.30 M potassium phosphate solution is combined with 20.00 mL of a 0.40 M solution 10. An Erlenmeyer flask is capped with a rubber stopper at room temperature (25 C) and atmospheric 11. The first step of the copper cycle lab was reacting solid copper with nitric acid. The copper ends up 12. What are the spectator ions in the 6 reactions performed during the copper cycle lab? for the reaction to cool and did NOT relight the "L-tube" flame. How would this affect your calculated percent mass compared to the true percent mass? of calcium chloride. What is the limiting reactant? What is the identity of the precipitate formed in the reaction? How many grams of product should be collected? pressure (1 atm). What temperature does the Erlenmeyer flask need to be heated to for the stopper to pop off? Assume it needs to exceed external pressure by 0.5 atm to release the stopper. oxidizing to copper (ll). What is the oxidizing reagent in this reaction? 13. The known specific heat capacity of aluminum is o g mo 25.316 g of aluminum is placed in 99.134 of water at a starting temperature of 22.45Â°C. The metal has a AT-84.02c what is the final 14. The AH, of cobalt (U) nitrate is +47.7 kJ/mol. What is the AHr of solid cobalt (1) nitrate? 15. 5.000 g of aluminum (Il) chloride is dissolved in 60.0 mL of water. The temperature changes by 16. Draw the Lewis dot symbols for the following atoms: temperature of the water? ÎÎ(Nouql)--205.00 kJ/mol ÎÎ,(Co2"m)--58.2 kJ/mol 0.331 Â°C. The specific heat capacity of aluminum (III) chloride is 0.903 Wat s AH.? what is ÎÎ a Ð°, Ð½Ðµ Ñ, Ñ c. Ar d. P e. H 17. Draw the Lewis structures for the following molecules: a. NHa b. O2 XeF d. NF

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Lab B4 Le ChÃ¢telier's Principle Introduction All chemical reactions proceed until equilibrium is reached, provided none of the reactants or the products are removed from the reaction mixture. Le ChÃ¢telier's principle describes what happens to an equilibrium after it has been disturbed (Ebbing/Gammon, Sections 14.7, 14.8, and 14.9). 05 Purpose You will study the application of Le ChÃ¢telier's principle by seeing the effect of the addition of Fe and SCN-to an equilibrium mixture of Fe", SCN, and Fe(SCN)ê³¼, the effect of the addition of an acid to an equilibrium mixture of Ni2, NHs, and Ni(NH)% the effect of the addition of an acid and a base on the equilibrium involving an indicator; the effect of acids and bases on the solubility of Ca(OH)2 in water and the effect of temperature on an equilibrium mixture of Co', cr, and CoCla 2- New Substances In this experiment you will encounter some substances that you may not have seen before. The reaction between Fe and SCN (thiocyanate ion) gives Fe(SCN)2. This substance is a deeply colored complex ion. Other complex ions that you will encounter are Ni(NHs)6 and CoCl These substances result from the reaction between Ni? and NH3 and from the reaction between Co and CI, respectively. You will also study an equilibrium involving methyl orange, an indicator. Indicators are discussed in Appendix D. Read the second, third, and fourth paragraphs of that appendix to gain an understanding of the physical and chemical properties of this indicator. Concept of the Experiment Le ChÃ¢telier's principle can be described in the following way: "When a system in chemical equilibrium is disturbed by a change of temperature, pressure, or concentration, the system shifts in equilibrium composition in a way that tends to counteract this change of variable" (Ebbing/Gammon, Section 14.7). This statement explains the effects that you will encounter in this experiment. Procedure lib Getting Started 1. Obtain 3 small test tubes and a piece of filter paper Obtain directions for discarding the solutions that you will use in this experiment from your laboratory instructor. Be careful handling the solutions used in this experiment. 2. 3. CAUTION: Solutions of ammonia, hydrochloric acid, and sodium hydroxide can cause chemical burns, in addition to ruining your clothing. Do not use your finger as a stopper when mixing these solutions. If you spill any of these solutions on you, wash the contaminated area thoroughly and immediately report the incident to your laboratory instructor. You may require further treatment. May not be scanned, copied or duplicated, or posted to a publily accessible website, in whole or in part be o 2013 Cengage Leaming All Rights Reserved. custom page 125