A student taught by Ms. Cook:__________________________ Period:________ Unit 6 Review: Topics 1-5 This packet is FOR YOU to learn since you will be taught the material directly FROM ME the teacher. There is homework at the end due on Friday 3/29/19 @ the door. Topics Reviewed: Topic 1: Specific Heat Capacity Topic 2: Heating Curves Topic 3: Heating Curve Calculations Topic 4: Calorimetry Topic 5: Solubility & Solubility Curves Monday 18 Topic 1 & 2 ET Topic 2 Due 25 Calorimetry Pre Lab Quiz Topic 4 Due Post Spring Break March 2019 – Unit 6 Calendar Tuesday Wednesday Thursday 19 20 21 Topic 3 Due No School Deer Park Ms. Cook out for PD. Fire No School Deer Park Fire 26 27 28 Calorimetry Lab ACT IA3 New Seats! Dismissal @ 12 Topics 1-5 Review Topic 5 Due April 2019 – Unit 6 Calendar Wednesday Thursday 3 4 Topic 6 Due Friday 22 No School Deer Park Fire 29 Monday 1 Tuesday 2 Ms. Cook Out Friday 5 HS IA Day No School 12 8 Ms. Cook out 9 English I EOC – Ms. Cook Proctoring 10 Topic 7 Due 11 English II EOC 15 Titration Lab 16 Titration Lab Topic 8 Due 17 Module 6 Review 18 Module 6 Exam 19 No School 22 Ms. Cook on NY Trip 23 Ms. Cook on NY Trip 24 Ms. Cook on NY Trip 25 Ms. Cook on NY Trip 26 Ms. Cook on NY Trip 29 30 1 2 3 A student taught by Ms. Cook:__________________________ Topic 1 Review: Specific Heat Calculating Specific Heat Period:________ Q = mc∆T, where Q = heat energy, m = mass, and ∆T = change in temp. Remember, ∆T = (Tfinal – Tinitial). Show all work and proper units. 1. A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron. 2. How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/g°C? 3. A 0.3 g piece of copper is heated and fashioned into a bracelet. The amount of energy transferred by heat to the copper is 66,300 J. If the specific heat of copper is 390 J/g 0C, what is the change of the copper's temperature? Topic 2 Review: Heating Curves Answer all the questions in complete sentences. 1. Label the phases (solid, liquid, gas) on the curve. 2. Label the phase changes (melting, boiling) on ethanol on the graph. 3. What is the melting point of ethanol? How do you know? 4. What is the boiling point of ethanol? How do you know? 5. In segment AB, explain what is happening to the molecules as heat is being added. 6. In segment BC, explain what is happening to the molecules as heat is being added. A student taught by Ms. Cook:__________________________ Topic 3: Heating Curve Calculations Period:________ 1. How much heat energy is required to raise the temperature of 15 g of Mercury from 40 °C to 80 °C? The specific heat capacity of Mercury is 0.671 J/g°C. a. The heat of vaporization of Mercury is 429 J/mol b. The heat of fusion of Mercury is 351.4 J/mol 2. How much heat energy is required to raise the temperature of 30 g of Iron from 1000 °C to 3500 °C? The specific heat capacity of iron is 0.172 J/g°C. a. The heat of vaporization of iron is 3070 J/mol b. The heat of fusion of iron is 1532 J/mol Topic 4: Calorimetry & Mixture Calorimetry Q = mc∆T, where Q = heat energy, m = mass, and ∆T = change in temp. Remember, ∆T = (Tfinal – Tinitial). Show all work and proper units. 1 C = 4184 J 1. How many Calories would be given off by 10.0 g of aluminum when its temperature changes from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/g°C? 2. How many Calories are required to heat 120.0 g of water from 2.0 °C to 24.0 °C? (C of H2O = 4.184 J/g °C) 3. To what temperature will a 50.0 g piece of glass raise if it absorbs 1.26 Calories and its specific heat capacity is 0.50 J/g°C? The initial temperature of the glass is 20.0°C. 4. Calculate the specific heat of a piece of wood if 1500.0 g of the wood absorbs 16.15 Calories and its temperature changes from 32°C to 57°C. (Mixture calorimetry) 5. A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal. A student taught by Ms. Cook:__________________________ Topic 4: Solutions Solute: Solvent: Heterogeneous – 2 types of mixtures Homogenous – Homogeneous Vs. Heterogeneous Practice 1. Flat soda pop 2. Cherry vanilla ice cream 3. salad dressing 4. sugar 5. soil 6. aluminum foil 7. black coffee 8. sugar water 9. city air 10. paint 11. alcohol 12. iron 13. beach sand 14. pure air 15. spaghetti sauce Period:________ Topic 5: Solubility 1. Label the following solutions as saturated, unsaturated, or supersaturated if 40 g of the substance is dissolved at 90 °C? AND say why you chose your answer. a. KI b. KNO3 c. NH3 d. NaCl Describe how to identify saturation: Saturated: Unsaturated: Supersaturated: 2. Label the following solutions as saturated, unsaturated, or supersaturated if 30 g of the substance is dissolved at 10 °C? Explain your reasoning using evidence from above and the graph. a. SO2 b. HCl c. NH4Cl d. KCl 3. A 100 g sample of water is saturated with NH4Cl at 50 °C. According to reference table G, if the temperature is dropped to 10 °C how many grams will fall out of solution? A student taught by Ms. Cook:__________________________ Period:________ Homework!!!! – Due 3/29/19 Topic 1 Specific Heat Calculations 1. Calculate the specific heat capacity of a piece of wood if 1500.0 g of the wood absorbs 67,500 joules of heat, and its temperature changes from 32°C to 57°C. 2. 100.0 g of 4.0°C water is heated until its temperature is 37°C. Calculate the amount of heat energy needed to cause this rise in temperature. 3. 25.0 g of mercury is heated from 25°C to 155°C and absorbs 455 joules of heat in the process. Calculate the specific heat capacity of mercury. 4. What is the specific heat capacity of silver metal if 55.00 g of the metal absorbs 47.3J of heat and the temperature rises 15.0°C? Topic 4: Calorimetry & Mixture Calorimetry 1. How many calories are required to raise the temperature of 67.0g of water from 25.7°C to 66.0°C? The specific heat of H2O is 4.184J/g°C) 2. What is the mass of a sample of metal that is heated from 58.8°C to 88.9°C with a specific heat of 0.4494J/g°C, if Q = 1.08 Calories 3. How many calories are required to raise the temperature of a 10.35g sample of carbon tetrachloride from 32.1°C to 56.4°C? The specific heat of carbon tetrachloride is 0.85651J/g°C. 4. A 5.00 g piece of metal is heated to 100.0oC, then placed in a beaker containing 20.0 g of water at 10.0oC. The temperature of the water rises to 15.0oC. Calculate the specific heat of the metal. Topic 2: Heating curves à Homework 1. Label the phases (solid, liquid, gas) on the curve. 2. Label the phase changes (melting, boiling) of the unknown substance on the graph. 3. What is the melting point of the substance? How do you know? 4. What is the boiling point of the substance? How do you know? 5. Given the chart to the below, identify the substance. Justify your answer. Sample Lead Potassium Sulfate Iron Silicon Dioxide Melting Point (°C) 328 1069 1538 1610 Boiling Point (°C) 1749 1689 2861 2230 A student taught by Ms. Cook:__________________________ Topic 3: Heating Curve Calculations à Homework Period:________ How much heat is required to raise the temperature of 25.0 g of NaCl from 60 °C to 100 °C? The specific heat capacity of water is 0.786 J/g°C. a. The heat of vaporization for water: 236 J b. The heat of fusion for water: 411 J 1. Label the curve with the phases (solid, liquid, gas) 2. Label the curve with the phase changes (melting, boiling) 3. At what temperature does NaCl melt? 4. What temperature does NaCl boil? 5. Draw a dot estimating where the initial temperature for the question is on the graph. 6. Draw a dot estimating where the finial temperature for the question is on the graph. 7. How many equations will you need to use to solve this problem? (Hint: count the numbers of sections between the initial and final temperatures) 8. Using the information given at the top of the question, solve for the heat required to produce the temperature change.