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Chemistry 2374A Lecture Notes - Lecture 9: Ideal Gas Law, Thermodynamic Equilibrium, Inexact Differential

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25 Dec 2017

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Western University

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Chemistry 2374A

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Document Summary

Chapter 2. 1 (cid:498)mathematical(cid:499) version of the first law. The internal energy of u of a system can be changed by heat (q) or work (w) The (cid:498)u(cid:499) is always in the system perspective; the system"s internal energy. The is for big change; d is for a small change. The internal energy u of a system can be changed by heat (cid:498)q(cid:499) or work (cid:498)w(cid:499) The ensuing combustion is highly exothermic, which releases heat therefore, internal. If work is positive, the work is going into the system; verse versa. If heat is positive, the heat is going into the system; verse versa energy is a state function (i. e. exact differential), while heat and work are path functions (i. e. inexact differentials) because integration must account for the path taken. For an infinitesimal change (small change) du = dq + dw d is used for an exact differential; d is used for an inexact differential.

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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.