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CHEM 123 Lecture Notes - Lecture 3: Ideal Gas Law, Path Dependence, Ideal Gas

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whitehedgehog343

11 Jan 2017

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Erin Lindenberg

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CHEM 123 Full Course Notes

CHEM 123 Full Course Notes

Document Summary

>learning goals: pistons, heat and work, measuring energy, heat capacity. >reversibility and irreversibility-characteristics of certain processes: reversible processes, property: system can be restored to its initial state without a net effect in the system/surroundings. 2: property: system cannot be restored to its initial state without a net effect in the system/surroundings. Note: for ideal gases, the internal energy is proportional to temperature. We want the gas to expand (do work on the system: reduce external pressure (pext), keep temperature constant. Path options (state 1 2 volume increased) Note: initial and final states are the same (from above) just take different path (different. Graph different amount of work area under graph) Extra: forward irreversible rxn = straight down from green and right to red: reversible process-remove slowly a. In equilibrium the entire time (ideal gas law, pv= nrt) i. ii. Amount of work out @ expansion = amount of work in @compression.

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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.