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CHEM 107 Lecture Notes - Lecture 17: Chemical Equation, Cross-Linked Polyethylene, Calorimetry

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8 Apr 2016

School

Texas A&M University

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Course

Professor

Hughbanks Timothy

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Document Summary

First law of thermodynamics: the energy of the universes is constant, delta e of the system + delta e of the surroundings = 0, delta e of the system = q + w. E is a state funcion but q and w are not state funcions q is speciic heat and w is work. Calorimetry: reacions are usually done at constant volume or constant pressure, measure q by measuring change in temperature, w= -pex*delta v. Enthalpy: h=e+pv, delta h= delta e + delta pv, delta h = q. Enthalpy and chemistry: delta h < 0 heat is released so reacion is exothermic, delta h > 0 heat is absorbed so reacion is endothermic. Formaion reacions: for any compound there is a formaion reacion. Elements in standard states 1 mole of compound: also called heat of formaion, always one mole of product so need to use fracional coeicients at imes, many such reacions cannot actually be carried out.

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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.