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CHEM 111 Chapter Notes - Chapter 10: Heat Capacity, Intensive And Extensive Properties, Heat Transfer

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13 Aug 2019

School

College of Charleston

Department

Chemistry and Biochemistry

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Professor

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Document Summary

Kinetic energy and potential energy are two broad classes of energy (10. 1a). Thermodynamics is the study of the relationships between heat, energy, and work (10. 1b). system (10. 1b). A change in internal energy is the sum of the work and heat added to or removed from a. Sign conventions are used to indicate the direction of heat and work flow between a system and the surroundings (10. 1b). The first law of thermodynamics states that the total energy for an isolated system is constant (10. 1b). Enthalpy is the sum of the internal energy of a system plus the product of pressure and. A change in enthalpy is equal to the heat exchanged between the system and surroundings at constant pressure (10. 2a). Heat is transferred from the system to the surroundings in an exothermic process (10. 2a). Heat is transferred from the surroundings to the system in an endothermic process (10. 2a). 10. 3 energy, temperature changes, and changes of state.

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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

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.