Chapter 9-3 Specific Heat Capacity

Slides:

Advertisements

Similar presentations

 Energy is transferred ◦ Exothermic – heat is released  Heat exits ◦ Endothermic – heat is required or absorbed by reaction  Measure energy in Joules.

Advertisements

Measuring and Using Energy Changes Section 20.2

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

THERMODYMANICS Thermodynamics is the study of the motion of heat energy as it is transferred from the system to the surrounding or from the surrounding.

Aim: How to measure molar heat of solution DO NOW: Get into groups of 3 or 4 and compare your homework. You have 5 minutes.

Warm-up… EXPLAIN HOW THE ICE CREAM LAB WORKS

THERMODYMANICS Thermodynamics is the study of the motion of heat energy as it is transferred from the system to the surrounding or from the surrounding.

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

Thermochemistry Unit Chapter 17. Problem #1 (page 664): A 92.0 g sample of a substance, with a temperature of 55 o C, is placed in a large scale polystyrene.

A calorimeter is used to measure the amount of heat absorbed or released during a chemical reaction.A calorimeter is used to measure the amount of heat.

Chapter 12 Changes in Temperature and Phases. Goals Perform calculations with specific heat capacity. Interpret the various sections of a heating curve.

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.

Specific Heat High School P. Science.

Reaction Energy and Reaction Kinetics Chapter 17 Notes.

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

E. Calorimetry q = m C  T q = heat or enthalpy J m = mass g C = specific heat J/g°C  T = temperature change °C Note – these problems could also be done.

Energy. ____________ – the ability to do work or produce heat ____________ energy – energy due to composition or position of an object ____________ energy.

Reaction Energy.

U3 S1 L3 Constant Pressure Calorimetry. Textbook Readings MHR pages : The Technology of Heat Measurement Textbook Practice Items MHR pages :

Heat Problems Calorimeter – an instrument used to study the heat of chemical reactions. Calorimetry – the study of the heat of chemical reactions.

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.

Challenge Problem If the density of an alloy of Al and Cd is 6.08g/cm 3, what is the % by mass and the % by volume of Al? The density of Al=2.70g/cm 3.

Energy Flow. Energy the ability to do work energy has no mass nor volume but is only detected by its effects thermochemistry studies energy changes during.

Specific Heat Capacity Every substance has it’s own specific heat because it has a different arrangement of atoms SubstanceSpecific Heat (J/g°C) Water4.18.

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

Thermodynamics Practice. Heat Absorbed/Released 1.How many joules of heat are needed to raise the temperature of 10.0 g of magnesium from 22°C to 55°C,

Specific Heat Practice. Gold has a specific heat of J/(g°C). How many joules of heat energy are required to raise the temperature of 15 grams of.

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

Worksheet Chapter Key. 1. Which substance must have more energy removed from it to undergo a ten degree temperature drop? One with a low specific.

Heat energy is measured in units called joules or calories. 1 calorie is the amount of heat energy needed to raise the temperature of 1.0 g (mL) of water.

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

Specific Heat Quantity of energy needed to increase the temperature of one gram of a substance by one degree Celsius/Kelvin Every substance has its own.

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

Heat Changes in Temperature and Phase. Specific Heat Capacity Specific heat capacity – the quantity of energy needed to raise the temperature of 1 kg.

1 This graph can be divided into 3 distinct regions, Identify them and explain what is occurring in each segment.

Chemistry Notes Energy and Heat Heat Capacity and Specific Heat.

ENERGY n The ability to do work n remains constant in amount during a chemical or physical change n energy changes occur between the system and the surrounding.

Chapter 17 Thermochemistry.

Specific Heat 4/28/17.

Chapter 10/11 Practice Test

© 2012 Pearson Education, Inc.

Specific Heat IB1 Chemistry

Specific Heat Capacity

Thermochemistry The study of the changes in heat energy that accompany chemical reactions and physical changes.

Specific Heat Problems

Thermochemistry The branch of chemistry concerned with the quantities of heat evolved or absorbed during chemical reactions.

Heat Unit 10 Lesson 1.

Welcome to the MATH.

Unit 04 - Heat Ht 1 03 – Energy Changes in one substance & Energy transfer using conduction.

Thermochemistry: Part 2

Hello! (January 10th) Pre-lab in lab books out, please!

Thermochemistry Specific Heat.

Reaction Energy.

Energy Content in Foods

Specific heat capacity

THERMOCHEMISTRY Thermochemistry is the study of the motion of heat energy as it is transferred from the system to the surrounding or from the surrounding.

Heat Unit 10 Lesson 1.

Specific Heat Calculations

Make a model-melting ice on two blocks

Specific Heat Capacity (比熱容量)

Calorimetry CP Unit 9 Chapter 17.

Thermochemistry The study of the changes in heat energy that accompany chemical reactions and physical changes.

Calorimetry Conservation of thermal energy: Final Temperature: m1 m2

Thermochemistry Chapter 17.

Specific Heat Specific heat – the quantity of energy needed to increase the temperature of one gram of a substance by 1 K or 1 ºC Every substance has its.

Ch.17: Reaction Energy and Reaction Kinetics

Thermochemistry The study of the changes in heat energy that accompany chemical reactions and physical changes.

Presentation transcript:

Chapter 9-3 Specific Heat Capacity St. Augustine Preparatory School January 12, 2017

Note: We will be doing a lab on calorimetry Monday and Tuesday. The lab report that will be completed will take place of the test for chapter 9. You will work in groups for the lab but the report will be done individually in a Google Doc.

Specific Heat Capacity: the amount of energy required to change the temperature of 1.0 kg of a substance by 1.0 degree Celsius. Formula: cp is specific heat capacity, with units: J/kg°C Q is the heat energy, with units: J m is the mass of the sample, with units: kg ΔT is the temperature, with units: °C

The heat water absorbs (Qw) is equal to the heat the object loses (Qx) In a closed system, the energy released by one object is equal to the energy absorbed by the other. Calorimetry: used to find heat changes in reactions, as well as specific heat capacities for different objects. We use water in calorimeters since we know the specific heat of water. Qw = -Qx The heat water absorbs (Qw) is equal to the heat the object loses (Qx)

Practice Problem: Suppose a piece of iron with a mass of 21 Practice Problem: Suppose a piece of iron with a mass of 21.5 g at a temp of 100.0 °C is dropped into an insulated container of water. The mass of the water is 132.0 g and its temperature before adding the iron is 20.0 °C. What will be the final temp of the system? Specific heat capacity of iron is 4.48x102 J/kg°C. Specific heat capacity of water is 4.186x103 J/kg°C.

A 12. 48 g sample of an unknown metal, heated to 99 A 12.48 g sample of an unknown metal, heated to 99.0 °C was then plunged into 50.0 mL of 25.0 °C water. The temperature of the water rose to 28.1 °C. Assuming no loss of energy to the surroundings: a. How many joules of energy did the water absorb? b. How many joules of energy did the metal lose? c. What is the specific heat capacity of metal?

What is the final temperature when a 3 What is the final temperature when a 3.0kg gold bar at 99 degrees Celsius is dropped into 0.22kg of water at 25 degrees Celsius. SHC of gold is 1.29x102 J/kg°C and the SHC of water is 4.186x103 J/kg°C.