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CHEM 123 Lecture Notes - Iodine Monochloride, Pentane, Isothermal Process

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14 Jul 2013

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CHEM 123 Full Course Notes

CHEM 123 Full Course Notes

Document Summary

First law of thermodynamics: a system expands and lifts a weight in its surroundings. How does this work affect the energy of the system: you have your hands wrapped around a system. The system changes state and produces a flux of heat at its boundaries. Is the change in enthalpy, h, associated with this change in state positive or negative: let us say that the apparatus of question 2 above consists of plastic cup containing water with solutes undergoing a chemical reaction. The water solvent forms part of the surroundings (as do the walls of the cup and the universe beyond. ) A thermometer in the solution shows the temperature dropping. How does this result for e compare with h for the same change in state: given the enthalpy changes at a certain temperature for reactions (a) and (b), calculate the enthalpy change for reaction (c). Is reaction (c) endothermic or exothermic at this temperature? (a) (b) (c)

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Related Questions

write and simplfy the closed system energy balance ( Equation : Q-W= delta U+ delta E_k+ delta E_p) for each of the follwing processes and state whether nonzero heat and work terms are positive or negative

a. the contects of a closed flask are heated from 25 celsius to 80 celsius

b. a tray filled with water at 25 celsius is pur into a freezer. the water turns into ice at -4 celsius. note: when a substance expands it does work on its surroundings and when it contracts with surroundings do work on it .

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.