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01:160:161 Chapter Notes - Chapter 9: Calorimeter, Kinetic Energy, Energy

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30 Dec 2019

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Rutgers University

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Document Summary

= a iters p v where m=mass (kg); v=velocity orce/area or f. Thermochemistry: the study of energy changes accompanying chemical and physical reactions. Energy: the potential to do work; the driving force of all changes. Energy can be in many forms: light, heat, work, electrical, etc. It can neither be destroyed nor created; it converts from one form to another at a fixed rate. System: the part/properties of which one wants to study. This could be the reaction vessel and its contents. Surrounding: the part of the universe (outside the system) with which the system interacts. Kinetic energy: the energy that a moving object possess. (meters/second) Potential energy: energy due to position (high or low) or composition of the system. Work: the force times the distance of the force; the manifestation of energy that becomes apparent during a process. Internal energy: the sum of all forms of energy: kinetic+potential.

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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.