DO NOW: On back of worksheet!!

Slides:

Advertisements

Similar presentations

Intro to thermochem - Discuss HEAT v. TEMPERATURE

Advertisements

Thermochemistry Part 2: Calorimetry.

Measuring and Using Energy Changes Section 20.2

Chapter 2 Heat Capacity and Specific Heat

Thermochemistry the study of the transfer of energy between reacting chemicals and their surroundings.

Reaction Energy and Reaction Kinetics Thermochemistry.

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

Energy in Chemical & Physical Changes

Thermochemistry Heat a form of energy. can be transferred between samples heat flows from matter at a higher temperature to matter at a lower temperature.

THERMOCHEMISTRYTHERMOCHEMISTRY Chapter 11. HEAT CAPACITY AND SPECIFIC HEAT The amount of energy needed to to increase the temperature of an object exactly.

Thermodynamics Ch 10 Energy Sections Thermodynamics The 1st Law of Thermodynamics The Law of Conservation of Energy is also known as The 1st.

Thermochem Jeopardy Exo/Endo Unit Conversions Vocab Specific Heat & Calorimetry Miscellaneous Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300.

Purpose: Have you ever wondered why some foods give you more energy than others? Background Information: Calorimetry is the study of finding the amount.

Thermochemistry Chapter 17.

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.

THERMO- CHEMISTRY Thermochemistry Study of the heat changes that occur during a chemical reaction.

CHAPTER 17 THERMOCHEMISTRY. ENERGY Energy is the capacity to do work or to supply heat. Various forms of energy include potential, kinetic, and heat.

Thermochemistry Some say the world will end in fire, Some say in ice, From what I’ve tasted of desire I hold with those who favor fire. Robert Frost Fire.

Thermochemistry. Do Now – Check and edit prelabs Objective – Thermochemistry Exothermic, endothermic, calorie, joule, heat capacity, and specific heat.

Ch. 15: Energy and Chemical Change

Thermochemistry Energy Heat Thermochemical Equations Calculating Enthalpy Change Reaction Sponteneity.

ENERGY AND CHEMICAL CHANGE Chapter 15. ENERGY ENERGY: -the ability to do work or produce heat. 2 different forms: potential and kinetic -Measured in.

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

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:

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.

Thermochemistry (The study of energy transfers) Mr. Forte Atascadero High School.

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

WARM UP 1.Given the thermochemical equation H 2 + I 2  2 HI, ΔH° rxn = 52 kJ/mol. What is ΔH° for the reaction HI  ½ H 2 + ½ I 2 ? 2.Given that the heat.

HW 5.4 a. 200 KJ b. by 4 c. Heat up brakes and road a.  E = q + w b. No energy is not gained or lost. c. System loses heat or does work on the surroundings.

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,

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

Section 10.2 The Flow of Energy 1.To convert between different energy units. 2.To understand the concept of heat capacity. 3.To solve problems using heat.

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

Ch.1: Matter and Change Introduction to Thermochemistry.

Thermochemistry.

Unit 13 Thermochemistry.

Chapter 17 – Thermochemistry

Heat capacity and Calorimetry

Thermochemistry.

Unit: Thermochemistry Chapter 16 in text

Specific Heat 4/28/17.

Specific Heat Calorimetry.

Chemistry 17.2.

Chapter 16: Energy and Chemical Change

Specific Heat Capacity

Matter and Energy 1.

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

Ch. 16 Thermochemistry Notes

Measuring Food Energy by Calorimetry

11.3 – NOTES Combustion.

Thermochemistry: Part 2

Thermochemistry Specific Heat.

DO NOW: (on the front of your WS)

Heat Capacity and Specific Heat

Energy Measuring Heat Calorimetry

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

Thermochemistry Lecture 1.

Thermochemistry.

Make a model-melting ice on two blocks

Thermochemistry Thermochemistry the study of the energy changes that accompany physical or chemical changes in matter. Changes may be classified.

Thermochemistry Feeling hot, hot, hot.

Topic 16: Energy and Chemical Change

17.2 Calorimetry Calorimetry is the precise measurement of the heat flow into or out of a system for chemical and physical processes.

DO NOW: On back of Notes! How much heat (in kJ) is given out when 85.0g of lead cools from 200.0C to 10.0C? (c=.129 J/gC)

Unit 5: Thermochemistry

DO NOW: (back of Notes) On a cold winter’s day you open the door to your house. Are you letting the cold in, or the heat out? How is the amount of calories.

Ch.17: Reaction Energy and Reaction Kinetics

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

Chemistry Quiz Ch 11 Section 11-1 & 11-2

Presentation transcript:

DO NOW: On back of worksheet!! The Calories in a McDonald’s Big Mac© is approximately 540. How many chemistry calories is this? How many kJ is this?

Unit: Thermochemistry Day 2 - Notes Unit: Thermochemistry Calorimetry and q=mcΔT

After today you will be able to… Describe what a calorimeter is and its function Explain what temperature change is dependant on Explain specific heat (c) and use the specific heat equation: q=mcΔT

Calorimetry: Is the accurate and precise measurement of heat change for chemical and physical processes. A calorimeter is a device used to measure the amount of heat absorbed or released during these processes. Example: Styrofoam cups! 

“Coffee Cup”Calorimeter: Constant-Pressure Calorimeter The thermometer records temperature change as the chemicals react in the water. The temperature change is then converted into units of energy. Most helpful for measuring the heat lost/gained in a chemical reaction.

Bomb Calorimeter: Constant-Volume Calorimeter A food sample is lit on fire. It burns until it is completely gone. Heat from the sample is released and heats up the water. The temperature change is then converted into units of energy. Most helpful in measuring the calorie content in food.

Temperature change is dependant on: Amount of heat added Mass of the substances Composition of the substance (specific heat) Example: Boiling water – metal pot gets hotter faster than water.

Specific heat: (c) amount of heat required to raise the temperature of 1 gram of a substance by 1˚C http://ga.water.usgs.gov/edu/heat-capacity.html

Units: Specific heat of H2O: cal J or g˚C g˚C 4.18 J/g˚C or 1.00 cal/g˚C

q=mcΔT q= m= c= ΔT= heat (J or cal) mass (grams) specific heat g˚C cal g˚C J specific heat or change in temperature (˚C) (Tfinal-Tinitial)

q= (525g) (0.21cal/g˚C) (34.8˚C) q= 3800cal Example: How many calories of heat are required to raise the temperature of 525g of aluminum from 13.0˚C to 47.8˚C? (cAl=0.21cal/g˚C) q= ? cal m= 525g c= 0.21cal/g˚C ΔT= 47.8-13.0= 34.8˚C q= (525g) (0.21cal/g˚C) (34.8˚C) q= 3800cal

5100cal= (m) (1.00cal/g˚C) (71.6˚C) m=71g Example: What mass of water would have its temperature raised from 22.5˚C to 94.1˚C with the addition of 5.1kcal of heat? 1000 cal q= 5.1 kcal x = 5100 cal 1 kcal m= ? g c= 1.00 cal/g˚C ΔT= 94.1-22.5= 71.6˚C 5100cal= (m) (1.00cal/g˚C) (71.6˚C) m=71g

Questions? Complete WS!

SILENCE IS GOLD-EN