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CHEM 130 Chapter Notes - Chapter 6: Exothermic Reaction, Limiting Reagent, Potential Energy

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27 Jan 2015

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Jadwiga Sipowska

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Potential energy: energy on an object has by virtue of its position in a field of force. Internal energy: the sum of the kinetic and potential energies of the particles making the substance. Law of conservation of energy: energy can be converted from one to another, but the total quantity of energy remains constant. Heat is defined as the energy that flows into or out of a system because of a difference in temperature between the thermodynamic system and its surroundings. Heat of reaction at a given temperature is the value of q required to return a system to the given temperature at the completion of the reaction. Exothermic reaction heat is evolved sign of q - . Endothermic reaction heat is absorbed sign of q + (bear in mind, combustion reaction, release heat, the sign for q is - ) At constant pressure q is writing as qp. p means constant pressure.

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Related Questions

1.) Which statement isincorrect?

(a) Energy is the capacity todo work or to transfer heat.

(b) Kinetic energy is theenergy of motion.

(c) Potential energy is the energy that a system possesses by virtue ofits position or composition.

(d) A process that absorbsenergy from its surroundings is called exothermic.

(e) The Law of Conservation of Energy is another statement of the FirstLaw of Thermodynamics.

2. Which of the following statementsabout the first law of thermodynamics and energy is false?

(a)Kinetic energy cannot be convertedto potential energy.

(b)Kinetic energy =1/2mv².

(c)All the energy in the universe isconserved.

(d)A system can never decrease itsenergy.

(e)Potential energy is the energy ofposition or composition.

3. Whichone of the following thermodynamic quantities isnot a state function?

(a)work (b) enthalpy (c)entropy (d) internalenergy (e) free energy

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.