01:160:161 Lecture Notes - Thermochemistry, Joule, Ionic Compound

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vsg20

13 Jul 2022

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Rutgers University

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Chemistry

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01:160:161

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Thermo thermochemistry = relationship between chemistry and energy deal with energy changes during chemical processes quantifying energy exchanges/transfers between chemical reactions and their surroundings. J, kj, cal, kcal or cal, l*atm [liter-atmosphere] **energy transfers always occur between system and surroundings internal energy (e) what"s the 1st law of thermo total energy of the universe is constant thermo2 mathematical equation. **don"t forget about the (+) and (-) signs internal energy of system (e) total energy of system sum of ke and pe of all particles state function. [value depends on current state of system and not how system arrives at state] state = specified by certain parameters " current temperature, pressure, etc. path function. Does depend on path that system goes to achieve a certain state internal energy change ( e) difference between initial state and final state = e (final) - e (initial)

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Two 20.0-g ice cubes at â12.0 Â°C are placed into 235 g of water at 25.0 Â°C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts.

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.

01:160:161 Lecture Notes - Thermochemistry, Joule, Ionic Compound

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