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Q1:SECTION 4 (AC4.1 / AC4.2) (A) For the following reactions, determine the equilibrium constant equation. You must show your workings within your submission. 1) CO₂(g) + H2(g) CO(g) + H₂O(g) 2) 2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g) 3) Cu(s) + 2Ag (g) Cu2*(g) + 2Ag(s) 4) H₂(g) + 1₂(g) 2HI(g) (B) Read the following relating to the Haber process: "The raw materials for this process are hydrogen and nitrogen. Hydrogen is obtained by reacting natural gas - methane - with steam, or through the cracking of oil. Nitrogen is obtained by burning hydrogen in air. Air is 80% nitrogen; nearly all the rest is oxygen. When hydrogen is burned in air, the oxygen combines with the hydrogen, leaving nitrogen behind. Nitrogen and hydrogen will react together under these conditions: A high temperature - about 450°C • A high pressure - about 200 atmospheres (200 times normal pressure) • An iron catalyst" The chemical reaction which occurs during the Haber process is: Nitrogen + Hydrogen → Ammonia N₂(g) + 3H₂(g) = 2NH3(g) 1. Explain Le Chatelier's principle. 2. Use Le Chatelier's principle to explain what would happen if you raised the temperature of this reaction. 3. Use Le Chatelier's principle to explain what would happen if you increased the pressure of this reaction. 4. Use Le Chatelier's principle to explain what would happen if used increased the concentration of Nitrogen at the start of the reaction. Your response for this question should be a maximum of 500 words.See Answer
Q2:SECTION 2 (AC2.1/AC2.2) (A) Imagine you have been given a series of materials to react together and the following enthalpy change data has been recorded. Explain the terms exothermic and endothermic, and identify which of the following are exothermic and endothermic reactions. Ensure that you explain your reasoning. Your explanation should be a maximum of 500 words. 1. N₂ + 20₂ → 2NO₂ AH = +68kJ mol-¹ 2. C3H8 +502 → 3CO2 + 4H₂O AH = -2220kJ mol-¹ AH = -486.3kJ mol-¹ AH = +566kJ mol-¹ 3. 2H₂ + O2 → 2H₂O 4. 2CO₂ → 2CO + + O₂ (B) You have been asked to calculate the enthalpy change in the following reaction: 2Al(s) + Fe2O3(S) → Al2O3(s) + 2Fe(s) The reaction occurs in the following stages: Chemical Change Assignment 1. 2Al(s) + Fe2O3(S) → Al2O3(s) + 2Fe(1) 2. Al₂O3(s) + 2Fe(1)→ Al2O3(s) + 2Fe(s) 3. Al2O3(s) + 2Fe(1)→ Al2O3(s) + 2Fe(s) Note stages 2 and 3 look the same, but the reaction is cooling from 1700°C to 25°C and hence the enthalpy change there. Calculate the overall enthalpy change for the reaction. You must show your workings within your submission, and explain your reasoning. Your explanation should be a maximum of 300 words. AH = -732.5kJ mol-¹ AH = -27.6kJ mol-¹ AH = -91kJ mol-¹ 1See Answer
Q3:SECTION 1 (AC1.1 / AC1.2) You will need to answer each of the questions in this section. You must include your full workings of your answers within your submission. 1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.221. 2. You have a sample which consists of 428g sodium hydroxide (NaOH) dissolved in enough water to make a final solution of 6.41. What is the molarity? 3. You have been given a sample of 4.85 moles of glucose (C6H12O6) and you want to make a 0.75M solution with it. What will be the final volume of solution? 4. 37.0cm³ of a sodium hydroxide (NaOH) solution was pipetted into a conical flask and titrated with a standard solution of 0.3 mol dm-³ hydrochloric acid according to the following equation: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(1) A universal indicator solution was used for the titration and it was found that 22.0 cm³ of the acid (HCI) was required to neutralise the alkali (NaOH). Calculate the molarity of the sodium hydroxide.See Answer
Q4:6- the formula of Titration is: MA = VA X MA nA Write the formula of MA, MB from it. MB= = VA = volume (cm³) of acid used M₁ concentration of acid no. of moles of acid in balanced egn for rxn n, V₂ X M₂ n₂ V₁ = volume (cm³) of base used M₂ - concentration of base ng no. of moles of base in balanced egn for rxnSee Answer
Q5:Determine the empirical formula of the oxide of magnesium. (Think carefully about the precision of each mass that you measured before you do this calculation. How many significant figures are justifled for each mass?) (3 Points) Write correctly balanced chemical equations for the following reactions: (4 points) a. Magnesium with molecular oxygen 2 M9102 2 Ngo b. Magnesium with molecular nitrogen c. Magnesium nitride with water Mga N₂ + 6H₂O →3 Mg(OH)₂ + 2NH3 d. Heating magnesium hydroxide Mg(OH)₂ →→ MgO + H₂O When 0.422 g of phosphorus is burned, 0.967 g of a white oxide is obtained. (3 Points) a. Determine the empirical formula of the oxide b. Write a balanced equation for the reaction of phosphorus and molecular oxygen on the f this empirical formula./nSee Answer
Q6:9) For each of the following compounds, use the solubility table to determine whether the compound would dissociate into ions or precipitate out as a solid (Write dissolve if it dissociates or precipitate if it forms a solid in the blanks provided) NaCl AgBr CaCO3 KOH Fe(NO3)2. BaSO4See Answer
Q7:8) Give the correct formula for the product(s) for each of the following chemical reactions, then in the blank to the right, give the type of chemical reaction that is occurring (combination, single replacement, double replacement, combustion of an organic, a) b) Li + N₂ c) d) e) Ca + 0₂ f) Fe(NO3)2 Na + HC1 + CuCl → KOH K C3H8 + 0₂ ↑ ↑See Answer
Q8:5-35. Calculate the "exact" alkalinity of the water in Problem 5-34 if the pH is 9.43.See Answer
Q9:5-34. Calculate the "approximate" alkalinity (in mg/L as CaCO3) of a water containing 120.0 mg/L of bicarbonate ion and 15.00 mg/L of carbonate ion.See Answer
Q10:5-29. Convert the following from mg/L as the ion or compound to mg/L as CaCO3: a. 200.00 mg/L HCI b. 280.00 mg/L CaO c. 123.45 mg/L Na₂CO3 d. 85.05 mg/L Ca(HCO3)₂ c. 19.90 mg/L Na*See Answer
Q11:5-28. Convert the following from mg/L as the ion to mg/L as CaCO3: a. 83.00 mg/L Ca²+ b. 27.00 mg/L Mg²+ c. 48.00 mg/L CO₂ (Hint: See footnote on p. 293) d. 220.00 mg/L HCO3 e. 15.00 mg/L CO ▾ Answer Ca²+ = 207.25 or 207.3 mg/L as CaCO, Mg²+ = 111.20 or 111.2 mg/L as CaCO3See Answer
Q12:5-20. What amount of NaOH (a strong base), in mg, would be required to neutralize the acid in Example 5-7? newerSee Answer
Q13:5-11. Calculate the mg/L of the following: a. 0.01000 N Ca²+ b. 1.000 M HCO, c. 0.02000 N H₂SO4 d. 0.02000 M SO²-See Answer
Q14:5.9. Calculate the molarity and normality of the following: a. 80 µg/L HNO3 b. 135 μµg/L CaCO, c. 10 µg/L Cr(OH), d. 1000 µg/L Ca(OH)₂See Answer
Q15:5-8. Calculate the molarity and normality of the following: a. 200.0 mg/L HC1 b. 150.0 mg/L H₂SO4 c. 100.0 mg/L Ca(HCO3)₂ d. 70.0 mg/L H₂PO4 Answer Molarity (M) Normality (N) 0.005485 a. 0.005485 b. 0.001529 0.003059 c. 0.0006168 0.001234See Answer
Q16:5-4. What is the concentration of chlorine (in mg/L) of household bleach that contains 5.25 percent by weight of Cl₂? Assume the density of water = 1,000 kg/m³.See Answer
Q17: Graded Assignment Unit Test, Part 2 Answer the questions below. When you have finished, submit this assignment to your teacher by the due date for full credit. For full credit, you must show all steps of your calculations. Scroll down to view the periodic table at the end of this document. (5 points) 1. Use the solubility curve to answer the following questions. Solubility vs. Temperature Score 100 90 NaNO3 Pb(NO3)2 KNO3 Solubility (g of salt in 100 g H20) 80 80 70 60 CaCl2 50 40 NaCl 30 20 10 % KCI KCIO3 K2Cr2O7 Ce2(SO4)3 10 20 30 40 50 60 70 80 90 100 Temperature (°C) a. Interpret the graph. What does it tell us about solubility? b. How much sodium chloride can dissolve in 80° C? C. Which substance shows a different trend than the others in its solubility? d. Mary dissolves the maximum amount of KNO3 possible into 100 grams of boiling water and then cools the solution quickly to a temperature of 12° Celsius. What is she likely to see? (5 points) 2. Rafiq dissolves 3.5 g of NaCl in 0.15 kg of water. The salt dissolves to form a solution of sodium and chloride ions.. What will the freezing point of the solution be? (Freezing- point depression constant for water is -1.85 C/m). Please be sure to provide all steps of your calculations for full credit. Stride, Inc. All rights reserved. No reproduction without written consent of Stride, Inc. Score Page 1 of 3 Graded Assignment (5 points) Science | Unit: Solutions | Lesson: Unit Test 3. In your own words, what happens at the molecular level when a solid dissolves into a liquid. Then, list three factors that we studied in this unit that influence the rate of solubility and how they do so. (5 points) 4. Consult the periodic table below and calculate the concentration of the solution. Be sure to include your units in your final answer. Mixtures Sample A Sample B Sample C Solute 16 g KCI 25 g NaCl 120 g O2 Solvent 0.4 L of water 100 g water 1350 g CO2 Concentration Molarity= Mass percent= Mole fraction of O2= O Stride, Inc. All rights reserved. No reproduction without written consent of Stride, Inc. Score Score Page 2 of 3 Period 7 Period 6 Period 5 Period 4 Period 3 Period 2 Period 1 Graded Assignment Group 1 1A Periodic Table Nonmetals Metalloids Noble gases Halogens Other nonmetals Science | Unit: Solutions | Lesson: Unit Test Group 18 8A Atomic number Metals 2 1 H Hydrogen 3 Cu Solid Ar Gas Alkali metals He Group 2 Symbol 1,0079 2A H Be Name Average atomic mass Hydrogen 1.0079 Br Liquid Am Not found in nature Alkaline earth metals Transition metals Other metals Group 13 ЗА Group 14 4A Group 15 5A Group 16 6A Group 17 7A 5 6 B F Helium 4.0026 10 Ne Lithium 6.941 Beryllium 9.0122 Boron 10.81 Carbon 12.011 Nitrogent 14.007 Oxygen 15.999 Fluorine 18.998 Neon 20.179 11 Na 22.990 12 Mg Magnesium 24.305 15 16 17 18 ΑΙ Si Ar Group 3 Group 4 Group 5 Group 6 3B 4B 5B 6B Group 7 7B Group 8 8B Group 9 9B Group 10 10B Group 11 11B Group 12 12B Aluminum 26.982 Silicon 28,086 Phosphorus 30.974 Sulfur 32.06 Chlorine Argon 35.453 39.948 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 Sc Ti Mn Fe Co Ni Cu Potassium Calcium Scandium 39.098 40.08 44.956 Titanium 47.90 Vanadium 50.941 Chromium 51.996 Manganese 54.938 Cobalt Copper Zn Ga Ge As Se Br Kr 55.847 58.933 58.71 63.546 65.38 Gallium 69.72 72.59 Arsenic 74.922 Selenium 78.96 Bromine 79.904 Krypton 83.80 38 39 41 42 43 45 46 47 48 50 51 52 53 54 Rb Sr Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Xe Rubidium 85,468 Strontium 87.62 Yttrium Zirconium 88.906 91.22 Niobium 92.906 Molybdenum Technetium 95.94 (98) Ruthenium 101.07 Rhodium 102.91 Palladium Silver 107.87 Cadmium 112.41 Indium 114.82 118.69 Antimony 121.75 Tellurium 127.60 lodine 126.90 Xenon 131.30 55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 Cs Ba Lu Hf Ta W Re Os Ir Pt Au Cesium Barium 132.91 137.33 Lutetium 174.97 Hafnium 178.49 Tantalum 180.95 Tungsten 183.85 Rhenium 186.21 Osmium 190.2 Iridium 192.22 Platinum 195.09 Gold 196.97 Mercury Thallium 200.59 204.32 Lead 207.2 Hg TI Pb Bi Po Polonium (209) At Rn Astatine (210) Bismuth 208.98 Radon (222) 87 88 103 104 105 106 107 108 109 110 111 112 114 Fr Ra Lr Rf Db Sg Bh Hs Mt Ds Rg Uub Francium (223) Radium (226) (262) (261) Lawrencium Rutherfordium Dubnium Seaborgium (263) (262) Bohrium (264) Hassium (265) Meitnerium (268) Darmstadtium Roentgenium (269) Ununbium (272) (277) Uuq Ununquadium When the average atomic mass is shown in parentheses, it means that this is the mass number of the most stable isotope. For these elements the average atomic mass cannot be determined. 57 58 59 60 61 62 63 64 65 Lanthanide Series La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho 67 68 69 70 Er Tm Yb Lanthanum 138.91 Cerium 140.12 Praseodymium Neodymium 140.91 144.24 89 90 91 92 Promethium (145) 93 Samarium 150.4 Europium 151.96 Gadolinium 157.25 Terbium 158.93 Dysprosium 162.50 Holmium 164.93 Erbium 167.26 Thulium 168.93 Ytterbium 173.04 94 95 96 97 98 99 100 101 102 Actinide Series Ac Th Pa U Am Cm Bk Cf Es Fm Md No Actinium (227) Thorium 232.04 Protactinium Uranium Neptunium Plutonium 231.04 238.03 (237) (244) Americium (243) Curium (247) Berkelium (247) Californium (251) Einsteinium (252) Fermium (257) Mendelevium (258) Nobelium (259) O Stride, Inc. All rights reserved. No reproduction without written consent of Stride, Inc. Your Score Click or tap here to enter text of 20 Page 3 of 3See Answer
Q18: Graded Assignment Unit Test, Part 2 Answer the questions below. You may use a scientific calculator for this test. When you have finished, submit this assignment to your teacher by the due date for full credit. 1. A chemist performs a titration to determine the concentration of a KOH solution. She places 24.0 mL of the solution into a flask and titrates it with 0.011 M HCI solution. A neutral endpoint once 14.6 mL of acid is added. Assuming the acid and base react completely, what is the initial concentration of the base? You must show all work for full credit. 2. Complete the calculations to fill in the table below. For full credit, you must show all calculations beneath the table. Substance Hydronium lon Concentration H+ Hydroxide lon Concentration OH- Ph Value Solution A Solution B Solution C 1.2 x 10-4 M 3.4 x 10-8 M 2.5 x 10-8 M Acid or Base? 3. A student is investigating the properties of an unknown acid, HA, and its dissociation in water. The student prepares a 0.1 M solution of HA and finds that the concentrations of H+ and A- ions in the solution to each be 1.5×10-2 M. What is the Ka for this substance? Be sure to show all steps of the calculation for full credit. 4. Calculate the volume of 0.550 M HCI solution needed to completely react with 25 mL of 1.30 x 10-2 M NaOH. Show all steps of the calculations.See Answer
Q19: Graded Assignment Part 2 1. Answer the questions below. Unless otherwise instructed, you may use a scientific calculator and refer to the periodic table in the Chemistry: Problems and Solutions book for this test. When you have finished, submit this assignment to your teacher by the due date for full credit. SHOW ALL WORK IN YOUR CALCULATIONS FOR FULL CREDIT. (6 points) A chemistry student is asked to identify a metal. He finds that 12-gram sample gains 26.0 joules of heat when it is heated from 100° C to 105.54º C. Perform calculations and consult the chart below to identify the metal. Score Click or tap here to enter text. Substance C (J/g-°C) Water (ice) 2.05 Iron 0.46 Aluminum 0.90 Gold 0.13 Copper 0.39 (7 points) 2. Study the image below and discuss what it represents and how the law of conservation of energy applies. Score Click or tap here to enter H reactants ΔΗ products text. Page 1 of 4 8 points) 3. For the following reaction, the enthalpy change is +44.6 KJ/mol. NHCl(s) = NH3(g) + HCl(g) Score Click or tap here to enter text. a. How much energy is absorbed when 50.0 g of ammonia chloride decomposes? You must show all steps of your calculations for full credit. b. Calculate the change in enthalpy during the reverse reaction to produce 70 g of ammonium chloride. Is energy absorbed or released? You must show all steps of your calculations for full credit. 4. Mrs. Gussman's van has a cooling system with a capacity of 9.45 liters. She filled the van with a coolant that has a specific heat capacity of 7.95 J/g–°C and a density of 1.114 g/mL. The van produced 58,500 kilojoules of heat during her drive to camp. The coolant temperature increases from 87° C to 105° C. How many times did the volume of coolant turn over its volume to maintain the engine temperature during this trip? Page 2 of 4 Page 4 of 4See Answer
Q20: Graded Assignment Name: Click or tap here to enter text. Graded Assignment Mid-Unit Test, Part 2 Science | Unit: Reaction Rates and Equilibrium | Lesson: Mid-Unit Test Date: Click or tap here to enter text. Answer the questions below. When you have finished, submit this assignment to your teacher by the due date for full credit. (8 points) 1. Use the diagram below to answer the following questions. Score activated complex Click or tap here enter text. ● Explain what this graph shows. Energy (a) reactants Reaction pathway • What is represented by the arrow labeled (a). • Is this reaction exothermic or endothermic? Explain how you know. Answer: Click or tap here to enter text. products (8 points) 2. The diagram below shows steps in a chemical reaction. Use the key below to determine the identity of the atoms. Score Color of sphere Identity of atom Red Oxygen White Hydrogen Blue Black Chlorine Carbon O Stride, Inc. All rights reserved. No reproduction without written consent of Stride, Inc. Click or tap here to enter text. Page 1 of 4 Graded Assignment A B Science | Unit: Reaction Rates and Equilibrium | Lesson: Mid-Unit Test C • • • Place the figures (A, B and C) in the correct order and describe what is happening at each step in detail. Write a balanced chemical equation to represent this reaction. Describe three ways that we can decrease the rate of reaction. Answer: (8 points) 3. Use the graph below to answer the questions below. reaction • • Answer: Rate of reaction Score with enzyme Click or tap here enter text. reaction without enzyme Concentration of substrate Discuss the information conveyed by the graph in terms of reaction rate. Using the information learned in your lessons, how does a catalyst work? O Stride, Inc. All rights reserved. No reproduction without written consent of Stride, Inc. Page 2 of 4 Graded Assignment (8 points) Science | Unit: Reaction Rates and Equilibrium | Lesson: Mid-Unit Test 4. Study the following graph and refer to it when answering the questions below: 100- Score Answer: Percent of reaction completed Time ||| 10°C 20°C 30°C a. Interpret the graph - what information does it convey? b. What does the slope of each line represent? Click or tap here to enter text. 5. Study the figure below and explain what information it conveys in your own words. Include a discussion of how the change in temperature affects the reactions rate. Use what you know about the energy of activation and collisions theory in your explanation of the graph. Answer: Number of particles T T+t Energy activation energy O Stride, Inc. All rights reserved. No reproduction without written consent of Stride, Inc. Page 3 of 4 Graded Assignment Science | Unit: Reaction Rates and Equilibrium | Lesson: Mid-Unit Test O Stride, Inc. All rights reserved. No reproduction without written consent of Stride, Inc. Click or tap here to enter text. Your Score of 40 Page 4 of 4See Answer

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