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BIOCHEM 2EE3 Lecture Notes - Thermodynamics, Enthalpy, Exergonic Process

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pearyellowjacket704

17 Mar 2014

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McMaster University

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Document Summary

Thermodynamics: studies relationship between heat and other forms of energy. 1st law of thermodynamics: the total amount of energy in the universe is constant, although the form of energy may change. Energy cannot be created or destroyed; only transferred into a different medium. System: part of the universe in question during thermodynamic analysis. The energy change of a system ( u) is the difference between heat (q) exchanged with the surroundings and the work (w) done by the system on the surroundings. Under constant pressure p, work is de ned by the volume change of the system. Enthalpy, h = q = u + pv. In most biochemical reactions, v is incredibly small, so h = u, or heat exchange approximates work done by the biochemical system. Spontaneous processes: occur without the input of energy. If all components of a reaction are at 1m concentration. Not necessarily the concentration in question and may differ from experimental conditions in question.

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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.