Specific Heat and Phase Change Ditto
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This document provides information and examples on calculating the heat energy required for specific heat and phase change problems involving water. It lists the specific heats of ice, liquid water, and water vapor. It then gives three example problems calculating the joules of energy needed to change the temperature of water and for phase changes between ice and water. Finally, it provides 11 practice problems for students to calculate the joules of energy required for various temperature changes and phase changes of water and ice of different masses.
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This document provides a study guide for a chapter 17 thermochemistry exam, including practice problems on thermochemical equations, heat capacities, enthalpy changes, and Hess's law. The problems cover topics like:
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Thermochemistry is the study of energy changes that occur during chemical reactions and phase changes. Heat (q) is energy that transfers from one object to another due to a temperature difference. Exothermic processes release heat (negative q value), while endothermic processes absorb heat (positive q value). Enthalpy (H) is the heat content of a system at constant pressure, and enthalpy changes (ΔH) quantify the heat absorbed or released during chemical reactions. Thermochemical equations relate the enthalpy change to the heat of reaction. Calorimetry problems use these equations and concepts to calculate energy changes involved in physical and chemical processes.
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1) Calorimetry can be used to measure the enthalpy change of reactions by using either a constant pressure calorimeter or a bomb calorimeter.
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Tang 01 heat capacity and calorimetry
1. Thermodynamics is the study of heat transfer and temperature changes that occur during physical and chemical processes.
2. The first law of thermodynamics states that the total energy in the universe is constant; energy cannot be created or destroyed, only transferred or changed in form.
3. Specific heat capacity is the amount of heat required to change the temperature of 1 gram of a substance by 1°C. Water has a unusually high specific heat capacity, allowing it to absorb large amounts of heat with only small temperature changes.
4. Calorimetry involves measuring heat changes that occur during chemical reactions. The heat transferred during exothermic reactions causes temperature increases, while endothermic reactions cause temperature decreases.
Heat in changes of state
The document discusses heat and phase changes. It defines key terms like heat of fusion and heat of vaporization, which refer to the energy required for a substance to change phases. The document also provides an example heating curve for 1 gram of water and uses equations like q=m*H to calculate energy changes during phase transitions. It gives examples of calculating the heat required to melt ice, condense a gas, and change ice to water over a temperature range.
Lecture 11 heat and phase changes
1) Heat is energy transferred due to a temperature difference without work. Specific heat is the amount of heat needed to change the temperature of a mass by a certain amount. Water has a very high specific heat.
2) Matter exists in solid, liquid, and gas phases. Phase changes involve a structural change of matter and absorb or release latent heat without changing temperature.
3) A phase diagram shows the relationships between pressure, temperature, and phases of a substance. The triple point is where solid, liquid, and gas phases coexist in equilibrium.
Thermochemistry ok1294993378
The document discusses energy changes that occur during chemical reactions. It defines exothermic and endothermic reactions, and standard enthalpy change. It provides examples of how to calculate enthalpy changes from experimental temperature change data using concepts like specific heat capacity. Hess's law, which states the enthalpy change of a reaction is equal to the sum of enthalpy changes of the steps in a reaction mechanism, is also introduced.
Tang 01 heat capacity and calorimetry
1. Thermodynamics is the study of heat transfer and temperature changes in chemical reactions and physical changes of matter.
2. The first law of thermodynamics states that energy is conserved in the universe and cannot be created or destroyed.
3. Calorimetry involves measuring heat changes that occur during chemical reactions using a calorimeter. Exothermic reactions release heat while endothermic reactions absorb heat.
General-Chemistry-2_q4_Chemical-Thermodynamics.pptx
Spontaneous processes are natural processes that proceed without external intervention, such as ripening of fruits or heat transfer from hot to cold. They are irreversible and can be exothermic or endothermic. Entropy is a measure of disorder in a system. Spontaneous processes generally increase the entropy or disorder of a system. The entropy change of a process can be calculated using the heat of the process and temperature. Standard entropy values allow calculation of entropy changes under standard conditions.
2 energy and heat Energy 101 fall 2015
This document provides an overview of the key concepts around energy that were covered in a lecture, including:
1. Energy is the ability to do work and is measured in Joules, while power is the rate at which work is done and is measured in Watts.
2. There are different units used to measure energy and power, including Joules, BTUs, Watt-hours, and Kilowatts.
3. Energy exists in different forms, including kinetic energy from motion and potential energy from position or chemical state, and energy is transformed between forms but not created or destroyed.
3. Heat is a special form of energy related to molecular motion, and temperature indicates the average kinetic
Phase changes
The document discusses phase changes between solid, liquid, and gas phases. It defines latent heat as the heat absorbed or released during a change of state without a change in temperature, such as the heat of fusion absorbed during melting or the heat of vaporization absorbed during boiling. The document provides examples of common phase changes like melting, freezing, condensation, vaporization, sublimation, and deposition. It also discusses using calorimetry to measure heat transfer during phase changes by ensuring energy is conserved. An example problem is given about using specific heats to calculate the mass of ice needed to lower the temperature of a glass and water system.
New chm-151-unit-9-power-points-140227172226-phpapp01
Thermochemistry deals with heat and energy changes during chemical and physical processes. There are several key concepts:
1) Enthalpy (H) is a measure of the total energy of a system at constant pressure. For reactions that do not involve large volume changes, the enthalpy change (ΔH) can approximate the energy change (ΔE).
2) Calorimetry experiments allow measurement of heat changes (q) through determination of temperature changes of reaction mixtures using their specific heats.
3) Hess's law states that the enthalpy change for a reaction is the same whether the process occurs in one step or multiple steps. Standard enthalpy changes (ΔH°) can
New chm 151_unit_9_power_points
Thermochemistry deals with the heat involved in chemical and physical changes. It is a branch of thermodynamics that studies energy and its transformations. Enthalpy (H) is a measure of the total energy of a system at constant pressure and can be used to determine the heat of a reaction. Calorimetry experiments allow measurement of heat changes through determination of temperature changes of a system and surroundings using equations such as q = cmΔT. Bomb calorimetry and coffee cup calorimetry are two common techniques used to directly measure the heat of chemical reactions.
Heat (Enthalply) Problem Set
This document contains a worksheet with 15 multiple choice and short answer questions about heat (enthalpy) concepts including:
1) The metric unit for heat energy is joules
2) Substances with higher specific heat constants are better able to conduct heat
3) Questions ask students to convert between Celsius and Kelvin temperatures and calculate heat transfer involving changes in temperature using specific heat and formulas.
4 calorimetry
Calorimetry involves measuring the heat transferred to or from a chemical reaction by using the heat transferred to raise the temperature of water. The enthalpy change of a reaction can be calculated using the formula: ΔH = mass of water x specific heat capacity of water x temperature change. This document provides the process for measuring enthalpy changes including using a calorimeter, allowing reactants to reach temperature of surroundings before mixing, measuring temperature change, and calculating enthalpy change using the formula. An example calculation is included.
Ch6 z5e thermo
The document discusses key concepts in thermodynamics including:
- Energy is the ability to do work and is conserved. It exists in the forms of heat and work.
- Enthalpy (H) is a state function that is the sum of a system's internal energy (E) and pressure-volume work (PV) at constant pressure.
- The first law of thermodynamics states that energy is constant in the universe and can be calculated as the heat (q) plus work (w) transferred to or from a system.
17.1 17.2 lecture slides
Thermochemistry is the study of energy changes that occur during chemical reactions and changes in state. Heat is energy that transfers from one object to another due to a temperature difference. In an endothermic process, the system gains heat from its surroundings, while in an exothermic process the system loses heat to its surroundings. Calorimetry allows for the precise measurement of heat flow during chemical and physical processes using an insulated calorimeter. The enthalpy change of a reaction, measured in kilojoules, can be determined from calorimetry experiments and represented in a thermochemical equation.
CHEMICAL THERMODYNAMICS (SPONTANEITY AND ENTROPY)
CHEMICAL THERMODYNAMICS
* Spontaneity and Entropy
* Second Law of Thermodynamics
* Gibbs Free Energy and Chemical Equilibrium
Clean ch06 lecture_7e
This document provides an overview of thermochemistry and calorimetry. It discusses:
1) Thermochemistry deals with the heat involved in chemical and physical changes. Energy can be transferred between a system and its surroundings as heat or work.
2) Enthalpy (H) is a measure of the total energy of a system at constant pressure. For reactions that do not involve large volume changes, change in enthalpy (ΔH) can approximate change in energy (ΔE).
3) Calorimetry involves measuring heat transfer during chemical or physical changes using devices like coffee cup calorimeters. The heat transferred (q) can be calculated using specific heat capacity (c), mass (
Heat transfer
The document discusses heat transfer and related concepts including:
1) Heat is energy in transit and its units like joules and calories
2) Sensible heat associated with temperature change and specific heat capacity
3) Latent heat associated with phase changes and calculation of heat involved
4) Properties of steam and using steam tables to find properties at given conditions
5) Concepts and equations related to heat exchangers like calculating heat transfer between hot and cold fluids
Matter Part C
The document discusses the different states of matter and changes between states. It includes:
1) Descriptions of solids, liquids, and gases in terms of particle arrangement, volume, shape, and interactions.
2) Explanations of changes in state like melting, freezing, evaporation, and condensation that occur when energy is added or removed from a substance.
3) A diagram of a heating curve showing how temperature changes as energy is added for different substances and states. Sections with no temperature change represent changes in state.
Y11 stoichiometry.pptx (3).pdf
Y11
STOICHIOMETRIC
RELATIONSHIPS
REACTING MASSES AND VOLUMES
The document discusses three main topics:
1) Stoichiometric relationships can be used to calculate reacting ratios by mass and gas volume using mole ratios from chemical equations.
2) The SI and other common units used for pressure, volume, and other measurements in stoichiometry problems.
3) The key steps and concepts involved in solving various types of stoichiometry problems involving moles, masses, volumes of gases, concentrations, limiting reactants, theoretical and experimental yields.
Similar to Specific Heat and Phase Change Ditto (20)
General-Chemistry-2_q4_Chemical-Thermodynamics.pptx
General-Chemistry-2_q4_Chemical-Thermodynamics.pptx
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More from West Hollow MS Ms. Gill
Welcome to Regents Earth Science
This document provides instructions for students on the first day of an Earth Science class. It includes directions for students to find and label their seat, make a name tag, and fill out an index card with personal information. The document outlines classroom rules and procedures, such as arriving on time, respecting others, and asking permission to move around the room. It also lists required class supplies, provides an overview of the units that will be covered during the year, and describes homework, lab, quiz, and test grading policies. General lab safety rules are outlined.
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Prologue np1 2012
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The document summarizes Earth's geologic history condensed into one calendar year. Key events include:
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This document is a note packet about plate tectonics, earthquakes, and volcanoes. It contains definitions of key vocabulary terms and explanations of plate tectonic concepts like continental drift, seafloor spreading, and plate boundary types. It also discusses mantle convection cells, hot spots, local evidence of crustal motions, and the two processes that cause earthquakes. The packet provides students with essential information about dynamic earth processes in 3 pages of outlined notes.
Earthquakes final
The document discusses dynamics of the Earth including evidence of crustal motions such as uplift and erosion that create mountains and sedimentary layers. It explains how marine fossils found in high elevations provide evidence of crustal movement over time. Earthquakes are described as being caused by the movement of tectonic plates and release of stress that builds in rocks, sending seismic waves that can be used to locate an earthquake's epicenter. The layers of the Earth are also outlined, with the crust varying in thickness and composition in different regions.
Plates ex2
The document is a plate tectonics exercise that asks students to calculate how far the Eurasian Plate will move in different time periods based on its rate of movement of 3 cm per year. It asks the direction the plate is moving, and then has the student calculate the distance after 100 years (300 cm), 1,000 years (3,000 cm), 1 million years (3,000,000 cm), and 1 billion years (30,000,000,000 cm).
Plates Lab
The document discusses the theory of the ancient supercontinent Pangea, which existed around 250 million years ago. All the continents were joined together in a "C" shape with a central sea called Tethys. Pangea's massive size meant dry inland areas and allowed animals to migrate between poles. The exercise has students cut out continents and try reconstructing Pangea, comparing their results to the provided reconstruction. Additional evidence like matching fossils and rock sequences between continents that were once joined supports the supercontinent theory.
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Dynamic Earth Note Packet
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Specific Heat and Phase Change Ditto
- 1. Name:___________________________________ Period: _____ Date:_____________ Unit 1: Energy Specific Heat and Phase Change Problems Specific Heats of Water (see ESRT) Ice – 2.11 Joules/g oC Liquid water – 4.18 Joules/g oC Water vapor(steam) – 2.0 Joules/g oC Directions: Read the follow three example problems then complete the practice problems. Show all work and units! Example Problem 1: How many Joules are needed to change 5 grams of water from 20 degrees C to 50 degrees C? Formula for temp change = Mass X change in temp X SH 5g x 30oC X 4.18 Joules/g /oC = 627 Joules Example Problem 2: How many Joules are needed to change 5 grams of ice to water? Formula for phase change = Mass X Latent heat of fusion 5g x334 Joules/g = 1670 Joules Example Problem 3: How many Joules are needed to raise the temperature of 10 grams of ice at O degrees C to liquid water at 15 degrees C? (This is a 3 part problem) Step 1: Phase change – Formula for phase change = mass x latent heat of fusion (melting) = 10g x 334J/g = 3340 Joules Step 2: Temperature change – Formula for temp change = mass x change in temp x SH(water) 10g x 15 degrees C x 4.18j/g/ oC = 627 Joules Step 3: Add answers from step 1 and step 2- Phase Change + Temperature Change 3340+ 627 =3967 Joules
- 2. Problem 1 : How many joules of heat energy must be added to 45 grams of liquid water to change the temperature from 20oC to 152oC water vapor? How many steps are in this problem? Show ALL work. Problem 2 : How many Joules of heat energy must be added to 70 grams of ice to change the temperature from -15oC to 175oC water vapor? How many steps are in this problem? Show All work. Problem 3: How many Joules of heat energy must be added to 20 grams of ice to change its temperature from -115oC to -4oC? How many steps? Show All work. Problem 4: How many Joules of heat energy must be added to 35 grams of water vapor to change its temperature from 115oC to 135oC? How many steps? Show all work.
- 3. Problem 5 : How many calories of heat energy are released when 55 grams of solid copper cools down from 195oC to 15oC? (No phase change) How many steps? Where do you find the SH of copper? Show all work. Problem 6: How many joules of heat energy must be added to 105 grams of liquid water to change the temperature from 10oC to 125oC water vapor? How many steps are in this problem? Show ALL work. Problem 7: How many Joules of heat energy must be added to 45 grams of ice to change the temperature from -45oC to 150oC water vapor? How many steps are in this problem? Show All work. Problem 8: How many Joules of heat energy must be added to 20 grams of ice to change its temperature from -115oC to 25oC? How many steps? Show All work.
- 4. Problem 9 : How many joules of heat energy must be added to 150 grams of liquid water to change the temperature from 60oC to 150oC water vapor? How many steps are in this problem? Show ALL work. Problem 10 : How many Joules of heat energy must be added to 80 grams of ice to change the temperature from -25oC to 130oC water vapor? How many steps are in this problem? Show All work. Problem 11: How many Joules of heat energy must be added to 20 grams of ice to change its temperature from -15oC to 60oC? How many steps? Show All work.