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CHM 1311 Lecture Notes - Lecture 13: Process Function, Thermodynamics, Bond Energy

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blackgoldfish265

17 Nov 2016

School

University of Ottawa

Department

Course

Professor

Matthew Lafreniere

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Document Summary

The quantitative study of energy transfers transformations. Where the energy goes and how much of it goes there. Boundary: imaginary separation that allows matter and/or energy to move. Surroundings: everything else we don"t care to study. Law of conservation of energy: energy is neither created nor destroyed in any process, but can be transferred from one body to another or transformed for one form to another. Heat(q): the change of thermal energy with surroundings. When a reaction releases energy: released energy may ow from the chemical system to surroundings. When a reaction absorbs energy: energy is likely to be suppled by a heat ow from the surroundings. Factors that effect changes in temperature: change in temp. depends on q, the amount of heat transferred, change in temp. depends on the direction of heat ow: If a substance absorbs heat, change in temp is greater then 0.

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Related Questions

Energy cannot be created nor destroyed, but it can be transferred between a reaction and its surroundings. The change in energy, Delta E, is positive if the reaction absorbs energy, and it is negative if the reaction releases energy. You may also see this expressed in terms of change in internal energy, Delta U. For the purposes of this question, Delta U and Delta E are equal. One way a reaction can transfer energy to or from the surroundings is by releasing or absorbing heat. A reaction can also transfer energy, in the form of work, through a change in volume. The total change in energy is the sum of the heat and work: Delta E = q + w At constant pressure, q = Delta H and w = -P Delta V and so Delta E = Delta H - P Delta V Assuming constant pressure, rank these reactions from most energy released by the system to most energy absorbed by the system, based on the following descriptions: Surroundings get colder and the system decreases in volume. Surroundings get hotter and the system expands in volume. Surroundings get hotter and the system decreases in volume. Surroundings get hotter and the system does not change in volume. Also assume that the magnitude of the volume and temperature changes are similar among the reactions. Rank from most energy released to most energy absorbed. To rank items as equivalent, overlap them. Energy cannot be created nor destroyed, but it can be transferred between a reaction and its surroundings. The change in energy, Delta E, is positive if the reaction absorbs energy, and it is negative if the reaction releases energy. You may also see this expressed in terms of change in internal energy, Delta U. For the purposes of this question, Delta U and Delta E are equal. One way a reaction can transfer energy to or from the surroundings is by releasing or absorbing heat. A reaction can also transfer energy, in the form of work, through a change in volume. The total change in energy is the sum of the heat and work: Delta E = q + w At constant pressure, q = Delta H and w = -P Delta V and so Delta E = Delta H - P Delta V A mole of X reacts at a constant pressure of 43.0 atm via the reaction X(g) + 4Y(g) - 2Z(g), Delta H degree = -75.0 kJ Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L Calculate the value of the total energy change. AE, in kilojoules. Express your answer with the appropriate units.