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CHEM 111 Lecture Notes - Lecture 9: Exothermic Process, Endothermic Process, Thermodynamics

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sapphirewhale473

27 Sep 2016

School

Binghamton University

Department

Course

Professor

Clarice Kelleher

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Document Summary

Chem 111 lecture 9 chapter 6 energy. Nature of energy: work is done to achieve motion against an opposing force, it is an ordered motion that is related to the temperature, work= (force) (distance) Its exo because water must release heat in order to freeze. What is the system: exchange of heat between things, where the surroundings (the rest of the universe) don"t affect the reaction, add more shit from slides, for example: glass beaker where different chemicals are mixed. Different types of energy: kinetic energy energy of motion. Example: ball falling downwards: potential energy any energy that is stored in the object. Doesn"t just apply to gravity, also it applies to chemical bonds and structures. Example: ball is held certain height: internal energy all of the energy that particles make up in the substance. Example: energy is stored in the structure of the compound (nacl) and it can be released by a chemical reaction.

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Related Questions

Match each definition with the correct term:

1. The substance undergoing a physical or chemical change

2. A process where heat is absorbed from the surroundings (energy of the system increases)

Temperature

heat

energy

work

system

poteinal energy

thermal energy

kenitic energy

exothermic

endothermic

surroudings

it is relatively easy to change the temperature of a substance tha

Experiment 11 ENTHALPY OF REACTION (HESS'S LAW) IDEAS Both the physical and biological worlds are characterized by a complex interplay of chemical reactions. In all chemical reactions, heat is released or absorbed. Combustion is one of the commonly observed chemical reactions accompanied by the evolution of heat energy, which may be harnessed of for such as the heating of homes, or which may be converted to other forms energy, such as mechanical energy in the steam engine or the internal combustion engine. One of the pioneering studies on the heat of chemical reactions was made by Lavoisier and ace in 1 Investigating the heat associated with various reactions, including combustion, they showed that each reaction was associated with a specific amount of heat and that the heat evolved in chemical reaction is equal to the heat absorbed in the reverse reaction. Lavoisier had proposed the modern theory of combustion as the combination of a substance with aygen. He also suggested the hypothesis that respiration is merely slow combustion. With Laplace, Lavoisier attempted to compare the quantity of heat given off by a burning candle with that given off by a live chicken. The quantity of heat was determined by measuring the quantity of ice that melted, in an insulated container, in the presence of the candle or the chicken. Little progress was made in thermochemistry until about fifty years later, when G. Hess (1802- 18500 studied heats of reaction in greater detail and stated the law a840) that bears his name: The heat evolved or absorbed in a chemical reaction is the same whether the process is accomplished in one step or in many. The law suggested, therefore, that both the reaction and the thermodynamic data could be treated algebraically. Although it was an empirical law when Hess proposed it, it was theoretically justified a few years later when the principle of conservation of energy was proposed. Hess's law can be illustrated by the following problem. Calculate the change in heat (AH) for the following reaction: 1. Mgo(s) 2H+(aq) Use the following information to solve the problem: AH- -35 kl/mole AH -56 kJ/mole 3, H+(aq) oHraq)