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CHM362H5 Lecture Notes - Lecture 3: Enthalpy, Isolated System, Thermodynamics

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2 Jan 2016

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Document Summary

Thermodynamics of biological systems: provides a macroscopic description of heat and energy flow in systems, allows determination of whether a chemical reaction is possible (i. e. spontaneous, need to consider the system and surroundings, 3 types of systems. The first law of thermodynamics: law of the conservation of energy, energy can be created or destroyed, but cam change from one form to another. Movement through some distance by application of a force = force x distance: u is a state function. Enthalpy: more useful function for biological systems, h = enthalpy; u = internal energy; p = pressure; v = volume. H = u + pv: enthalpy is a state function. H = u + pv + p v: at constant pressure (case for biochemical reactions), pv = 0, recall that mechanical work is +w = -p v. Internal energy and enthalpy in biological systems: biological processes often occur in solids and liquids, rather than gases; v ~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.