combinations yields a precipitate. None of these combinations yields a precipitate. 7. (0.5 marks) Is the reaction below a precipitation‚ an acid-base or an oxidation-reduction reaction? Assume the reaction occurs in aqueous solution. CuSO4 + Zn → Cu + ZnSO4 A. B. C. a precipitation reaction an acid-base reaction an oxidation-reduction reaction 8. (0.5 marks) What is the percentage by mass of oxygen in UO2? Molar masses (in g mol−1) A. B. C. D. 33% 12% 6.7% 67% U‚ 238.0 O‚ 16.00 CHEM
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CHAPTER 4 REACTIONS IN AQUEOUS SOLUTION MULTIPLE CHOICE QUESTIONS 4.1 Which of the following compounds is a strong electrolyte? E A. H2O B. O2 C. H2SO4 D. C6H12O6 (glucose) E. CH3COOH (acetic acid) Answer: C 4.2 Which of the following compounds is a strong electrolyte? E A. H2O B. N2 C. KOH D. C2H6O (ethanol) E. CH3COOH (acetic acid) Answer: C 4.3 Which of the following compounds is a weak electrolyte? E A. HCl B. CH3COOH (acetic acid)
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Experiment 1: Calorimetry Nadya Patrica E. Sauza‚ Jelica D. Estacio Institute of Chemistry‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines Results and Discussion Eight Styrofoam ball calorimeters were calibrated. Five milliliters of 1M hydrochloric acid (HCl) was reacted with 10 ml of 1M sodium hydroxide (NaOH) in each calorimeter. The temperature before and after the reaction were recorded; the change in temperature (∆T) was calculated by subtracting the initial temperature
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GENERAL CHEMISTRY Laboratory Guide This module provides a laboratory guidelines‚ safety declaration form‚ Lab Report guidelines and Laboratory manual for subject of General Chemistry (CLD 10004). Mohd Zulkhairi Abdul Rahim Laboratory Information Before each lab session‚ you should prepare by reading the lab manual and the textbook required reading. We expect you to have a good understanding of the purpose‚ details of the procedure‚ the use of all chemicals and any significant hazards
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Data collection and processing Qualitative observation Before * Blue solution of copper sulfate * Grey zinc powder During * Blue color solution changes to greyish black * Heat is given out‚ so the surroundings become hotter. After * Grey powder remains on the sides of the cup * Precipitate formed at the bottom of the cup List of chemicals and apparatus used Chemicals used Copper sulfate solution‚ 1 mol dm-3 25g of zinc powder Apparatus needed
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appears to be “steam” comes off out of container. | single-displacement reaction | Zn + 2 HCl (aq) --> ZnCl2(aq) + H2(g) | 3. Black smoke occurs | decomposition reactions | 2 (H2O2)(aq) MnO2 2 (H2O) + (O2) | 4. reddish-brown deposit on the surface of iron; surface of the iron is found corroded; the blue solution turns light green | single-displacement reaction | Fe + CuSO4(aq) --> FeSO4 + Cu | 5. PbSO4 (milk white) | double-displacement reaction | Pb(NO3 )2(aq) + H2SO4(aq)
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bus 9.2 – Production of Materials: Δ. Construct word and balanced formulae equations of all chemical reactions as they are encountered in this module: • Basic reactions to remember: – Acid reactions: ▪ acid + base [pic] salt + water HCl(aq) + NaOH(aq) [pic]NaCl(s) + H2O(l) ▪ acid + metal [pic] salt + hydrogen gas HCl(aq) + Mg(s)[pic]MgCl2(s) + H2 (g) ▪ acid + carbonate [pic] salt + carbon dioxide gas + water HCl(aq) + CaCO3(s)[pic] CaCl(s) + CO2(g) + H2O
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Mike Morrison – SCH3U Types of Chemical Reactions Lab Intro/Purpose The purpose of this lab is to determine types of reactions with only the reactants and through observation. Through observing the experiments‚ one is able to see a visual of each type of reaction taking place and it gives them a better understanding of how chemical reactions work and what products they may form. Materials & Procedure Materials: * Wood Splints - Copper Sulfate * Sodium Sulfate - Copper
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) +2OH-(aq.) ---- Cu(OH)2 (s) 2Cu2+(aq.)+SO42- (aq.) +2NH3(aq.)+2 H2O(l) ----- Cu(OH)2.CuSO4(s) +2NH4+ (aq.) Zn2+ (aq.)+ 2OH- (aq.) ---- Zn(OH)2 (s) Zn2+ (aq.)+2NH3(aq.)+ H2O(l) --- Ag2O (s)+ 2NH4+ (aq.) Fe3+ (aq.)+ 3OH- (aq.) ---- Fe(OH)3(s) Fe3+ (aq.)+ 3NH3(aq.)+ 3H2O(l) --- Fe(OH)3(s)+ 3NH4+ (aq.) Pb2+(aq.)+ CrO42-(aq.) PbCrO4(s) 2Cu2+(aq.)+[Fe(CN)6]4- (aq.) -----Cu2[Fe(CN)6] (s) Zn2+(aq.) + S2-(aq) ----- ZnS(s) 4Fe3+ (aq.)+3[Fe(CN)6]4-
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following from strongest oxidizing agent to weakest oxidizing agent: Ce4+ Ce3+ Fe2+ Fe3+ Mg2+ Mg Ni2+ Sn 17.3: Cell Potential and Equilibrium ∆G=-nFEº Example: Using the data in table 17.1‚ calculate ∆Gº for the reaction: Cu2+ (aq) + Fe(s) Cu(s) + Fe2+ (aq) 17.4: The Nernst Equation What happens when concentration and temperatures are not standard? Nernst Equation Sometimes written as: Assuming 25ºC Example 1: What is
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