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CHEM 123 Lecture 2: CHEM 123 LEC 2 UBC CHEMISTRY THERMODYNAMICS WINTER 2019

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23 Feb 2019

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CHEM 123 Full Course Notes

CHEM 123 Full Course Notes

Document Summary

The first law of thermodynamics: conservation of energy: energy can neither be created nor destroyed, but it can be converted from one form to another. There exists a state variable called internal energy e. E is the sum of all forms of energy in the system. Change in energy (e) = q + w (for all paths) Internal energy: e[j], an extensive property: for any kind of energy. Change in energy = ef ei: equation of state for ideal gas, ideal gas isotherm. Internal energy (e): all forms of energy within a system, it includes. P1v1=p2v2: movement of molecules, translational, rotational, movement, energy within the molecule, vibrational, bonds, energy associated with the interactions between molecules, potential energy \ Internal energy of ideal gas: e of the ideal gas (pv=nrt) is a fxn of temperature only. For an ideal gas, if delta t=0, then delta e=0: for monatomic ideal gas,

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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.