SCH4U Thermochemistry Test Review Try all the problems previously assigned‚ look at the problems in your textbook‚ and try these: 1. Be sure to understand the following vocabulary: Thermochemistry Thermochemical Equation System Surrounding Calorimetry calorimeter Heat temperature thermal energy chemical energy Open‚ closed‚ isolated/insulated systems enthalpy change Molar enthalpy Exothermic changes Endothermic changes Hess’s Law Heat capacity specific heat capacity combustion
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Purpose: The purpose of the experiment is to calculate the enthalpy change occurring in the first of reaction of sodium hydroxide with hydrochloric acid and sodium hydroxide with ammonium chloride. Using Hess’ Law and the results for the enthalpy change of the first two reactions should give the enthalpy change of the third reaction of ammonia with hydrochloric acid. Procedure: Part 1: Construct a calorimeter of two nested stereophony cups where the cover has a hole to fir a thermometer. Measure
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Thermochemistry Laboratory Report Abstract The purposes of these three experiments are to determine the heat capacity of a calorimeter and with that data‚ confirm Hess’s Law and observe enthalpy changes within reactions. By measuring the change in temperature that occurs with the interaction of two different reactants‚ we were able to determine both the calorimeter constant and the change in enthalpy of a given reaction. The results were rather mixed‚ as some numbers more closely resembled the
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Thermochemistry Thermochemistry is the study of heat evolved and absorbed during the chemical reactions. The system is the interest of the universe; the surroundings are the rest of the universe in which the exchange of the energy with the system takes place. Both‚ the system and the surroundings make up the universe. Heat flow is the transfer of heat from a warm place to a cooler one. System to surroundings: Surroundings to system:
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Thermochemistry Lab #2 - Heat of Reaction - Hess’s Law Return The foundation of the study of thermochemistry was laid by the chemist Germain Hess‚ who investigated heat in chemical reactions during the last century. One statement of the law that bears Hess’s name says: The enthalpy change for any reaction depends on the products and reactants and is independent of the pathway or the number of steps between the reactant and product. In this experiment‚ you will measure and compare
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SCH4U UNIT 3: Thermochemistry Assignment May 2‚ 2011 1. Upon the addition of potassium nitrate to liquid water‚ the beaker feels cold. Explain‚ using appropriate terms: system‚ surroundings‚ heat‚ temperature‚ endothermic or exothermic. The endothermic process whereby the system of KNO3 crystals dissolving in the water absorb energy from the surroundings and the measured temperature of the surroundings (beaker‚ air) drops. 2. The phase change from
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Thermochemistry: An Ice Calorimeter Determination of Reaction Enthalpy Curtis M. Franklin Thursday‚ February 14‚ 2013 ABSTRACT An ice calorimetric measurement was used to determine that a reaction involving solid magnesium metal and 1.00M sulfuric acid produces an experimental a value of ∆H = -226 ± 28 kJ/mol at 0°C. This is about 48.4% lower than the expected value reported at 25°C. Introduction Many chemical reactions exhibit themselves by exchanging heat energy‚ either be absorbing
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Thermochemistry: An Ice Calorimeter Determination of Reaction Enthalpy Shannon Wedepohl 9/17/13 Abstract: During this experiment‚ an ice calorimeter was used to measure the change in volume in milliliters of magnesium metal and 1.00 M of sulfuric acid. We found the experimental molar enthalpy of the reaction to be ∆H = -370 ± 1 kJ/mol at 0˚C. This compares with an expected value of -466.9 kJ/mol at 25 ˚C‚ a 20.75% difference. Introduction: Many chemical reactions truly only
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Introduction The primary objective of this lab is to be able to determine the specific heat of a reaction by using a calorimeter. A calorimeter is a device used to determine the specific heat of chemical reaction or a physical change. The specific heat a reactions is used to refer to the amount of heat that is lost or gained when one gram of a particular substance increases or decreases by one degree Celsius. When a chemical reaction occurs in an open container most of the energy gained or lost
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Objectives: 1. Distinguish between system and surroundings. 2. Distinguish between heat energy and temperature. Name the SI units of temperature and thermal energy. 3. Calculate the heat content (thermal energy) of a substance using its specific heat‚ temperature and mass. 4. Solve calorimetry problems. 5. Name the energy associated with a change of state and calculate the energy required to change a given mass of substance from solid to liquid or liquid to gas. 6. Describe the changes in the microscopic
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