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CHEM 120A Lecture Notes - Lecture 10: Thermochemistry, Kinetic Energy, Potential Energy

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amaranthlion961

15 Dec 2016

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Department

Chemistry and Biochemistry

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Professor

Sachel Villafañe- Garcia

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Document Summary

According to the law of conservation of energy, energy can neither be created or destroyed in a reaction. System: a point of reference: in thermochemistry, reactions will be the system studied. Surroundings: the environment surrounding the system that can exchange energy: if something leaves the system, it goes to the surroundings, a system plus its surroundings is the universe. State functions do not depend on the path taken: real-life example: you need to climb a mountain but have se(cid:448)eral paths of doi(cid:374)g so. It does(cid:374)"t (cid:373)atter (cid:449)hich o(cid:374)e you take since they will all take you up: back to chemistry: internal energy is the sum of the kinetic and potential energy of the system. The change in internal energy of a system only constitutes the energy at the end of the reaction subtracted by the energy at the beginning of the reaction. It can also be thought of as the difference in energy between the products and reactants.

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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.