Warm-up… EXPLAIN HOW THE ICE CREAM LAB WORKS

Slides:

Advertisements

Similar presentations

Thermochemistry Part 2: Calorimetry.

Advertisements

Chapter 10 Energy. Chapter 10 Table of Contents Copyright © Cengage Learning. All rights reserved The Nature of Energy 10.2 Temperature and Heat.

Chemistry 312: Spring Review Endo v. Exo HW Endo v. Exo Pre Lab Questions Endo v. Exo Lab Notes on Specific Heat HW: Complete Lab Analysis Questions.

Measuring and Using Energy Changes Section 20.2

Section 15.2 Heat Describe how a calorimeter is used to measure energy that is absorbed or released. Explain the meaning of enthalpy and enthalpy change.

EQ: Describe the parts and each part’s function in a calorimeter?

Heat in chemical reactions

Exothermic and Endothermic Processes Essentially all chemical reactions and changes in physical state involve either: a) release of heat, or b) absorption.

Laboratory 12 CALORIMETRY. Objectives 1.Construct and utilize a coffee cup calorimeter to measure heat changes 2.Determine the heat capacity of a calorimeter.

What is the relationship between heat and temperature?

Calorimetry Chapter 5. Calorimetry Since we cannot know the exact enthalpy of the reactants and products, we measure  H through calorimetry, the measurement.

Unit 2 – Matter and Energy Mrs. Callender. Lesson Essential Question: What is Thermochemistry?

Warmup 1) Solve for x 689 = (1.8)(x)(45.2 – 27.4) 689 = (1.8)(x)(17.8) 2) On a hot summer afternoon, you get into the car, and it’s unbearably HOT inside!

What’s the MATTER: Specific Heat of Matter

Thermodynamics – chapter 17 Organic Chemistry –chapters 22 & 24

Warmup Given the following equations: H 3 BO 3(aq)  HBO 2(aq) + H 2 O (l) ΔH rxn = kJ H 2 B 4 O 7(aq) + H 2 O (l)  4HBO 2(aq) ΔH rxn = kJ.

Enthalpy Enthalpy is a measure of the total energy of a system. Enthalpy is a state function (the pathway does not matter) with the symbol H. H = E + P.

THERMOCHEMISTRY REVIEW You need a marker board, marker, eraser, & your Chemistry book.

Part One Heat and Temperature.

Energy and energy transformations. First Law of Thermodynamics  Energy is never created nor destroyed Energy can change forms, but the quantity is always.

Measuring and Using Energy Changes Section Main Idea Energy stored in chemical bonds can be converted to other forms and used to meet the needs.

1. The universe is made up of: The system – the thing that you are studying The surroundings- everything else 2.

THERMOCHEMISTRY Energy Enthalpy Specific Heat Calorimetry Phase Changes.

1 THERMOCHEMISTRY or Thermodynamics. 2 Energy & Chemistry ENERGY is the capacity to do work or transfer heat. HEAT is the form of energy that flows between.

Ch. 15: Energy and Chemical Change

Thermochemistry Energy Heat Thermochemical Equations Calculating Enthalpy Change Reaction Sponteneity.

Heat and Temperature. The difference Heat – the energy that flows from hot to cold. Measured in Joules (J) or calories (cal). Temperature – measure of.

Chapter 15.4 & 15.5 ENTHALPY AND CALORIMETRY.  Thermochemistry = heat changes that accompany chemical reactions and phase changes  Energy released 

 Energy – the ability to do work or produce heat ◦ Kinetic energy – energy of motion ◦ Potential energy – stored energy  Chemical potential energy –

Reaction Energy.

Thermodynamics X Unit 9. Energy: Basic Principles  Thermodynamics – the study of energy changes  Energy – the ability to do work or produce heat Note:

THERMOCHEMISTRY Specific Heat Thermochemistry 17.1  Thermochemistry is the study of energy changes (HEAT) that occur during chemical reactions and changes.

Specific Heat & Phase Changes. Specific Heat ____________ (c) – the amount of heat required to raise the temperature of 1 g of a substance 1 °C The units.

Chapter 11 Notes II Calorimetry. What is calorimetry? Essentially, the science of measuring heat change. At its most simple, you use the specific heat.

What’s the MATTER: Specific Heat of Matter. Matter, Specific Heat of Matter At the conclusion of our time together, you should be able to: 1. Define specific.

Reaction Energy Specific Heat u The specific heat of any substance is the amount of heat required to raise the temperature of one gram of that substance.

Heat Transfer and Calorimetry Dr. Keith Baessler.

Thermodynamics The study of the changes of heat in chemical reactions.

ENERGY AND CHEMICAL CHANGE CH. 16 Energy is the ability to do work or produce heat and is found in two forms potential energy is energy due to the composition.

Energy exits in two basic forms, ____________________ and ____________________ energy.

Energy change that occurs during a chemical reaction and/or changes in state.

Back Chapter 16 Reaction Energy West Valley High School General Chemistry Mr. Mata.

Energy Chapter 15 Mr. Smith’s favorite definition for chemistry How energy interacts with matter.

Energy Potential energy- energy of position or composition. Potential energy- energy of position or composition. Kinetic energy- energy of motion Kinetic.

 Different substances require different amounts of heat to change their temperature.  Objects that require more energy have a high heat capacity like.

Measurement of Heat Energy. The amount of heat given off or absorbed in a reaction can be calculated by a) q=mc∆T(Table T) q= heat (in joules or calories)

REACTION ENERGY CHAPTER 16 PAGE 500. A. THERMOCHEMISTRY 1. Introduction a. Every chemical reaction causes a change in energy b. Endothermic or exothermic.

CHM 101/102 Laboratory Manual Calorimetry. CHM 101/102 Laboratory Manual Calorimetry Background Background  The thermal energy (q) transferred when an.

Thermochemistry: Energy and Heat The Nature of Energy u Energy is the ability to do work or produce heat. u It exists in two basic forms, potential energy.

Chapter 17 – Thermochemistry

Chapter 17 Thermochemistry.

© 2012 Pearson Education, Inc.

Specific Heat Calorimetry.

THERMOCHEMISTRY.

Welcome to the MATH.

Thermochemistry Part 2: Calorimetry.

Reaction Energy.

Section 7.2—Calorimetry & Heat Capacity

VOCAB REVIEW… Potential Energy - energy due to position or composition

Chapter 16 Thermochemistry

Chapter 9-3 Specific Heat Capacity

Calorimetry Thermochemistry pt2.

Thermochemistry Lecture 1.

Make a model-melting ice on two blocks

Calorimetry CP Unit 9 Chapter 17.

Chapter Six: THERMOCHEMISTRY.

Ch.17: Reaction Energy and Reaction Kinetics

Presentation transcript:

Warm-up… EXPLAIN HOW THE ICE CREAM LAB WORKS What does the salt do (collig. Pro and temp gap) How does the ice melt– explain the heat movement

Calorimetry CP Unit 9 Chapter 17

CALORIMETRY The enthalpy change associated with a chemical reaction or process can be determined experimentally. Measure the heat gained or lost during a reaction at CONSTANT pressure

Calorimeter Device used to measure the heat absorbed or released during a chemical or physical process Styrofoam cup

Example If you leave your keys and your chemistry book sitting in the sun on a hot summer day, which one is hotter? Why is there a difference in temperature between the two objects?

Because… Different substances have different specific heats (amount of energy needed to raise the temperature of 1 g of a substance by 1 degree Celsius).

Need to know how to calc. heat (review) Heat (q) = mCT If the specific heat of Al is 0.90 J/gC, how much heat is required to raise the temperature of 10,000 g of Al from 25.0 C to 30.0 C? HIDDEN

Calculator says 45,000 J BUT 1 sig fig… HIDDEN

For example (review): HIDDEN If 418 J is required to increase the temperature of 50.0 g of water by 2.0 C, what is the specific heat of water? HIDDEN

What happens in a calorimeter One object will LOSE heat, and the other will ABSORB the heat System loses heat to surroundings = EXO = -q System absorbs heat from surroundings = ENDO = +q When a hot chunk of metal is dropped in a cool glass of water, the metal cools off. Where did the heat from the metal go? Did the metal lose more heat then the water gained? HEAT GAINED = HEAT LOST (ALWAYS!)

To do calorimetry problems… The numbers in these two boxes are always the same, but with different signs (+/-). What heat one lost, the other gained. Make a Chart: Water Object/Reaction Heat Mass Specific Heat 4.184 Final Temp Initial Temp

EXAMPLE: A small pebble is heated and placed in a foam cup calorimeter containing 25.0 g of water at 25.0 C. The water reaches a maximum temperature of 26.4 C. How many joules of heat were released by the pebble? The specific heat of water is 4.184 J/g C. (#13) Water Pebble Heat Mass Specific Heat 4.184 Final Temp Initial Temp The numbers in these two boxes are always the same, but with different signs (+/-). What heat one lost, the other gained. 25.0 g 26.4 oC 25.0 oC

The pebble because the water heated up from 25.0 C to 26.4 C. Pebble loses heat (-q, exothermic) while water gains heat (+q, endothermic) Do you calculation based on water (since the problem gave all the water’s information) 

Water Pebble Heat Mass Specific Heat 4.184 Final Temp Initial Temp 25.0 g 26.4 oC 25.0 oC qwater = mwatercwaterTwater qwater = (25.0g)(4.184J/goC)(26.4oC-25.0oC) qwater = 150 J If the water ABSORBED 150 J of heat, then the pebble _______ ______ J of heat. qpebble = - 150 J

Example 2 (LAB type of CALC) Suppose that 100.00 g of water at 22.4 °C is placed in a calorimeter. A 75.25 g sample of Al is removed from boiling water at a temperature of 99.3 °C and quickly placed in a calorimeter. The substances reach a final temperature of 32.9 °C . Determine the SPECIFIC HEAT of the metal.The specific heat of water is 4.184 J/g C.  MAKE YOUR CHART

Suppose that 100. 00 g of water at 22. 4 °C is placed in a calorimeter Suppose that 100.00 g of water at 22.4 °C is placed in a calorimeter. A 75.25 g sample of Al is removed from boiling water at a temperature of 99.3 °C and quickly placed in a calorimeter. The substances reach a final temperature of 32.9 °C . Determine the SPECIFIC HEAT of the metal.The specific heat of water is 4.184 J/g C. Make chart Calculate q for water Q for water is the same (but with different sign) as q for metal. Using q metal, calculate c metal Water Pebble Heat Mass Specific Heat 4.184 Final Temp Initial Temp 100.00 g 75.25 g 32.9 oC 32.9 oC 22.4 oC 99.3 oC

0.879 J/g °C

Example 3 A lead mass is heated and placed in a foam cup calorimeter containing 40.0 g of water at 17C. The water reaches a temperature of 20.0 C. How many joules of heat were released by the lead? The specific heat of water is 4.184 J/g C.

502 J = 5.0 x 102 J for 2 sig figs